Jhemical  Experiment!' 


General  and      uivtical 


Yv'illiams 


i  of  Olivias  Lry 


LIBRARY 

OF  THE 

UNIVERSITY  OF  CALIFORNIA 

01  FT  OP" 


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Accession  No.£>     Sl5~~£  .       C/<25S  A/b 


CHEMICAL   EXPERIMENTS 


GENERAL  AND  ANALYTICAL 


FOR    USE    WITH    ANY    TEXT-BOOK    OF    CHEMISTRY,    OR 
WITHOUT   A   TEXT-BOOK 


K.  P.  WILLIAMS 

Nx 

Instructor  in  Chemistry,  English  High  School,  Boston,  and 

Author  of  "  Introduction  to  Chemical  Science," 

"  Laboratory  Manual,"  etc. 


OS  t 

t_ 
„.  _  .  __ 


BOSTON,  U.S.A.,  AND  LONDON 

PUBLISHED  BY   GINN   &   COMPANY 

1895 


COPYRIGHT,  1895 
BY  R.  P.  WILLIAMS 


ALL  BIGHTS  RESERVED 


PEEFAOE. 


THE  rapid  growth  of  the  laboratory  method  of  teaching  chem- 
istry since  the  author's  Manual  was  issued  in  1888  has  called  for  a 
larger  and  more  comprehensive  work  of  a  similar  sort  for  high 
schools,  academies,  and  colleges.  To  such  a  call  tfre  present  book 
is  a  response. 

In  preparing  the  experiments  the  author  has  endeavored,  first, 
to  select  such  as  are  most  instructive  and  best  illustrate  the  subject 
without  being  too  elaborate ;  second,  to  arrange  them  in  an  order 
calculated  to  lead  up  by  the  most  natural  and  easiest  steps  to  a 
knowledge  of  the  science ;  third,  to  make  the  subject  fascinating 
by  giving  just  enough  information  and  suggestion  to  interest  the 
experimenter,  and  to  make  him  work  for  the  knowledge  to  be 
gained.  Finally,  the  author  has  aimed  to  make  the  book  simple 
enough  for  the  dull  and  slow  pupil,  and  —  by  the  introduction  of 
supplementary  and  original  work  —  elaborate  enough  for  the  most 
acute.  Great  care  has  been  taken  to  give  minute  and  accurate 
directions  for  performing  the  experiments.  "  Terms  "  at  the  end 
of  experiments  are  for  pupils  to  study  outside  the  laboratory,  and 
are  often  repeated.  They  may  also  be  discussed  in  the  laboratory. 

Metal  analysis  has  received  a  somewhat  unique  treatment. 
Each  metal  of  a  group  is  first  taken  separately,  and  the  analytical 
reactions  are  given.  This  method  shows  the  pupil  at  once  why  a 
given  re-agent  is  added,  and  what  its  effect  is.  The  product  is 
given  when  the  substance  is  in  solution  as  well  as  when  it  is 
precipitated.  The  group  is  next  treated  in  the  same  way.  This 
method  clarifies  the  subject  greatly  in  the  pupil's  mind,  and  is 
believed  to  be  a  valuable  departure  in  teaching  analysis. 


iv  PREFACE. 

The  new  orthography  recommended  by  the  Chemical  Section 
of  the  A.  A.  A.  S.  has  been  adopted,  as  a  step  towards  uniformity 
and  progress. 

It  is  recommended  that  wherever  it  is  possible  each  laboratory 
period  cover  the  space  of  two  hours  (even  if  there  can  be  only  one 
period  per  week),  and  that  the  last  20  or  30  minutes  be  taken  to 
question  the  class  rapidly  on  the  work  of  the  day,  discuss  and 
explain  the  use  of  terms,  etc.  The  books  should  be  inspected 
after  each  exercise,  or  perhaps  after  each  experiment  has  been 
written  out. 

It  is  by  no  means  necessary  to  perform  every  experiment,  or  to 
follow  the  order  here  given,  if  the  teacher  prefers  to  do  otherwise. 
A  diversity  of  opinion  exists  among  teachers,  and  a  diversity  of 
time  and  talent  among  pupils  and  classes.  In  no  place  better  than 
in  the  laboratory,  under  a  competent  instructor,  can  a  "  cast-iron 
rule  "  be  done  away  with,  and  variety  of  arrangement  and  method 
be  adopted. 

The  author  would  be  glad  to  receive  criticisms,  as  well  as 
suggestions  as  to  other  methods,  or  experiments,  or  different  ways 
of  performing  experiments.  Especially  would  he  be  glad  to  know 
what  it  has  been  difficult,  in  the  matter  of  directions  or  principles, 
for  pupils  to  understand. 

The  author  desires  to  acknowledge  valuable  suggestions  in  the 
preparation  of  this  work  from  the  following  persons  :  Messrs.  J.  Y. 
Bergen,  Jr.,  C.  W.  Gerould,  E.  F.  Holden,  A.  S.  Perkins,  K  S. 
French,  H.  I.  Lord,  E.  S.  Chapin ;  and  Misses  D.  M.  Stickney, 
M.  L.  Foster,  and  others. 

CAMBRIDGE, 

December  1,  1895. 


INDIVIDUAL   APPARATUS. 


Each  pupil  should  be  provided  with  the  apparatus  given  below,  but  in  cases 
where  great  economy  must  be  exercised  different  pupils  may,  by  working  at 
different  times,  use  the  same  set.  The  author  has  selected  apparatus  specially 
adapted,  as  to  exact  dimensions,  quality,  and  cheapness,  for  performing  in  the 
best  way  the  experiments  herein  described,  and  sets  or  separate  pieces  of  this, 
together  with  other  apparatus  and  chemicals,  can  be  had  of  the  L.  E.  Knott 
Apparatus  Co.,  14  Ashburton  Place,  Boston,  to  which  firm  teachers  are  referred 
for  catalogs. 


4  re-agent  bottles,  250  cc.  glass  stop- 
pers, blown  labels:  NH4OH, 
HC1,  HNO3,  H2S04. 

1  pneumatic  trough. 

1  Hessian  crucible. 

2  beakers. 

2  pieces  wire  gauze. 

1  piece  platinum  wire. 

1  mouth  blowpipe. 

6  pieces  glass  tubing. 

4  pieces  hard  glass  tubing. 

1  test-tube  brush. 

1  small  tube  brush. 

1  doz.  test  tubes. 

4  cork  stoppers,  for  tubes. 

1  fish-tail    attachment    for    Bunsen 

burner. 

1  blowpipe  attachment  with  rest  for 
Bunsen  burner. 

piece  sheet  copper. 

glass  retort. 

tumbler. 

piece  cobalt  glass. 

horn  spatula. 

sheet  litmus  paper. 
00  filter  papers. 

bunch  splints. 

sheet  turmeric  paper. 


1  camel's-hair  brush. 

1  magnet. 

4  wide-mouthed  bottles. 

1  2-holed  rubber  stopper  to  fit  above. 

4  pieces  window-glass. 

glass  funnel. 

porcelain  evap.  dish. 

asbestos  board. 

sand  bath. 

pair  iron  forceps. 

triangular  file. 

round  file. 

piece  copper  wire. 
1  piece  lead  wire. 
1  piece  zinc  wire. 
1  wooden  test-tube  holder. 
1  wire  test-tube  rack. 
1  thistle  tube. 
1  Bohemian  flask. 
1  2-holed  rubber  stopper  to  fit  flask. 


Bunsen  burner, 
iron  ring  stand. 


2  ft.  rubber  tubing. 
1  ft.      "          " 
1  metric  ruler. 
1  graduate. 
1  small  leaden  dish. 


GENERAL   APPARATUS. 


The  requirements  of  general  apparatus  for  a  laboratory  are  too  numerous 
and  varied  to  be  given  here.  A  few  of  the  pieces  in  more  general  demand  for 
experiments  in  this  book  are  as  follows : 


Glass-stoppered  bottles. 

Graduates. 

Funnels. 

Fruit  jars  (for  making  solutions). 

Scales,  with  metric  weights. 

Ignition  tubes. 

Beakers. 


Filter-stands. 

Glass  and  rubber  tubing. 

Steel  glass-cutters. 

Steel  wire-cutters. 

Mortars  and  pestles. 

Flasks. 

Filter  papers,  etc.,  etc. 


CHEMICALS. 

ESTIMATE  FOR  A  CLASS  OF  TWENTY  IN  GENERAL  CHEMISTRY  AND  ANALYTICAL 
REACTIONS,  NOT  INCLUDING  GENERAL  REACTIONS  AND  SUPPLEMENTARY 
WORK. 


Acid,  acetic,  HC2H3O2 4  Ib. 

"      boric,  H3B03 i  " 

"      hydrochloric,  HC1 25  " 

"      hydrofluoric,  HF i  " 

"      hydrofluosilicic,  H2SiF6....  i  " 

"      nitric,  HNO3 12  " 

"      oxalic,  H2C204 f  " 

"      phosphoric,  H3PO4 J  " 

"      sulfuric,  H2S04 18  " 

"      tartaric,  H2C4H406 i  " 

Alcohol,  C2H5OH 1  qt. 

Alum,  K2A12(SO4)4 1  Ib. 

Aluminum  chlorid,  A1C13 -J-  " 

Ammonium  carbon.,  (NH4)2C03  1  " 

chlorid,  NH4C1 2  " 

"  hydroxid,  NH4OH..20  " 

"  nitrate,  NH4NO3 1  " 

"  oxalate,  (NH4)2C204  i  " 

"  sulfate,  (NH4)2S04..  i  " 

Antimony  cryst.,  Sb ^  "  ' 

"         chlorid,  SbCl3 i  " 

Arsenious  oxid,  As4O6 1  oz. 


Arsenopyrite,  FeAsS Jib. 

Barium  chlorid,  BaCl2 i  " 

"  hydroxid,  Ba(OH)2 i  " 

Bismuth  oxychlorid,  BiOCl i  " 

Calcium  chlorid,  CaCl2 i  «' 

"  fluorid,  powdered,  CaF2  k  " 
"  hypochlorite,  CaCl20....  i  " 

"  sulfate,  CaS04 i  " 

"  oxid,  CaO 2  " 

Carbon  bisulfid,  CS2 i  » 

Charcoal,  animal,  gran.,  C 1  " 

•'  "  powdered,  C..  1  " 
"  wood,  u  C..  1  " 
«*  «»  C 20  pieces 

Cobalt  chlorid,  CoCl2 i  Ib. 


"      nitrate,  Co(N03)2 .... 

Cochineal 

Copper,  turnings,  Cu 

"       sheet,  Cu i 

"      chlorid,  CuCl2 1 

"       nitrate,  Cu(NO3)2 i 

**       oxid,  CuO 1 


i  " 
i  " 
3  " 


VI 


CHEMICALS. 


Vii 


Copper  sulfate,  CuSO4 i  Ib. 

Ether,  (C2H5)20 i  " 

Gold  leaf,  Au 1  bk. 

Indigo i  Ib. 

lodin,  1 2oz. 

Iron,  fine  turnings,  Fe 1  Ib. 

"     by  hydrogen,  Fe , -J-  " 

"     perchlorid,  FeCl3 1  " 

"     protosulfid,  FeS 5  " 

"     pyrite,  FeS2 i  " 

"     sulfate,  FeSO4 1  " 

Lead,  sheet,  Pb 1  " 

"      wire,  i  in.  diam.,  Pb 12  ft. 

"     acetate,  Pb(C2H302)2 i  Ib. 

"      chlorid,  PbCl2 i  " 

"     nitrate,  Pb(N03)2 2  " 

"      protoxid,  PbO i  " 

"     tetroxid  (red),  Pb304 i  " 

Litmus,  cubes 1  oz. 

Marble  chips,  CaC03 3  Ib. 

Magnesium  ribbon,  Mg 10  ft. 

"          chlorid,  MgCl2 i  Ib. 

sulfate,  MgSO4 £  " 

Manganese  chlorid,  MnCl2 £  " 

"          dioxid,  gran.,  Mn02..  £  " 
"      powd.,Mn02  li  " 

Mercury,  Hg $  " 

"        bichlorid,  HgCl2 £  " 

"        protochlorid,  HgCl £  " 

"        pernitrate,  Hg(N03)2....  i  " 
"        protonitrate,  HgN03....  i  " 

"        oxid,  HgO 1  " 

Nessler's  sol i  " 

Phosphorus,  P 2  oz. 

Picture  wire 1  roll 

Platinum  chlorid,  sol.,  PtCl4 loz. 

Potassium,  metallic,  K £  " 

"          bromid,  KBr ±  Ib. 

"          carbonate,  K2C03 1-J-  " 

"          chlorid,  KI £  " 

u          chlorate,  KC1O3 2  " 

"          chromate,  K2CrO4....  i  " 
"          cyanid,  KCN £  " 


Potassium,  dichromate,  K2Cr2O7  1  Ib. 
"  ferrocy.,  K4Fe(CN)6..  1  " 
«'  ferricy.,  K3Fe(CN)6..  f  " 

iodid,KI 1  " 

"          hydroxid,  KOH 1  " 

"          nitrate,  KN03 1  " 

u          nitrite,  KN02 i  " 

*'  permangan.,  KMnO4  i  " 
"  sulfocyanid,  KSCN....  i  " 
"  tartrate,  K2C4H406....  i  " 

Silica,  powdered,  Si02 i  " 

Silver  nitrate,  AgNO3 4  oz. 

Sodium,  metallic,  Na fa  " 

"       acetate,  NaC2H3O2 i  Ib. 

.  "       arsenite,  HNa2As03 |  " 

"       bicarbonate,  HNaC03....  i  " 

"       bisulfate,  HNaS04 i  « 

"       borate,  Na2B4O7 -J-  " 

"       carbonate,  Na2C03 3  «* 

"       chlorid,  NaCl 4  " 

u       hydroxid  (caust.),NaOH  3  " 

"       nitrate,  NaNO3 2  " 

"       nitrite,  NaNO2 -J-  «« 

«*       oxalate,  Na2C2O4 \  " 

"       phosphate,  HNa2P04 1  " 

sulfate,  Na2S04 

"       sulfid,  Na2S 

"       sulfite,  Na2S03 

"       thiosulfate,  Na2S203 

Starch,  C6Hi0O5 

Strontium  chlorid,  SrCl2 

Sugar,  Ci2H22On 

Sulfur,  brimstone,  S 2  " 

**      flowers,  S 1  «« 

Tin  bichlorid,  SnCl2 i  " 

Turmeric  paper 1  sheet 

Turpentine,  Ci0Hi6 loz. 

Zinc,  gran.,  Zn 3  Ib. 

"     wire,  i  in.  diam 12ft. 

"     (arsenic-free) lib. 

"     chlorid,  ZnCl2 i  " 

u     nitrate,  Zn(N03)2 i  u 

««     Litmus  paper i  quire 


1  » 

I  " 

i  " 

1  " 

i  " 
i" 

1  " 


SOLUTIONS,  ETC. 

In  making  solutions  for  metal  analysis,  chlorids  of  the  metals  are  usually 
taken  (except  in  Group  I,  in  which  nitrates  are  used,  the  chlorids  being  insol- 
uble). From  25  e  to  50  &  of  solids  are  usually  dissolved  hi  500 cc  of  distilled 
water,  and  filtered  if  necessary.  Many  are  sat.,  as  Ca(O  H)2.  Substances  for 
analysis,  as  well  as  acids  and  other  re-agents,  should  be  C.  P.  Concentrated 
acids  are  used  unless  the  dilute  are  called  for. 
A  few  exceptional  sols,  are  given  below  : 

HNa2P04,  40.  (NH4)2C03,  100.  (NH4)2S04,     5. 

KCy,  50.  KNO2,  50.  NH4C1,          60. 

K2Cr207,     25.  KOH,  60.  NaOH,          60. 

Dilute  acids  are  made  by  mixing  one  volume  of  concentrated  acid  with  four 

volumes  of  water. 
NH4OH.     If  NH4OH  of  26°  is  obtained,  it  should  be  diluted  with  three  times  its 

volume  of  water  before  using. 
HgN03  is  best  prepared  by  putting  into  a  large  e.d.  say  25s  of  Hg,  and  adding 

to  it  a  mixture  of  25 cc  HNO3  and  25 cc  of  H2O,  and  letting  it  stand  till 

action  stops,  then  adding  400 cc  or  500 cc  of  H2O.     More  Hg  should  be  used 

than  will  dissolve,  and  some  should  be  left  in  the  bottle. 
PbCl2  is  only  slightly  soluble  in  water.     A  saturated  sol.  should  be  used. 
BiClg  is  prepared  by  adding  water  and  HC1  to  oxychlorid  of  bismuth,  BiOCl. 

First  add  the  H2O,  then  acidulate  it  with  the  acid,  say  1  vol.  of  H  Cl  to  20 

of  H2O,  it  being  insol.  in  H2O  alone. 
AsCls.    Add  H20  to  sodium  arsenite  HNa2AsO3,  then  add  HC1  with  stirring  till 

effervescence  stops. 
SbCl3.    Pour  a  little  butter  of  antimony,  SbCl3,  into  H20,  then  acidulate  with 

HC1. 
SnC^.    This  must  also  be  acidulated  with  HC1,  and  a  little  Sn  should  be  left  hi 

the  bottom  of  the  bottle. 
CrCl3,    This  may  be  made  from  K2Cr207  sol.  by  adding  some  HC1  (say  ^)  and  a 

little  alcohol,  boiling  some  time  and  letting  it  stand,  when  it  turns  from  red 

to  green. 
(NH4)2S.    Pass  H2S  gas  into  dilute  NH4OH  till  the  sol.  gives  no  ppt.  with 

MgSO4  sol.,  then  filter.     It  should  be  nearly  colorless. 
(NH4)2SX  (ammonium  polysulfid).     Stir  sulfur  flowers  in  the  (NH4)2S,  as  above 

prepared,  then  filter.     It  is  yellow. 
Cochineal  sol,     Grind  up  a  handful  of  cochineal  in  a  mortar,  and  add  water,  stir, 

and  filter. 

Litmus  sol.    Pulverize  litmus  cubes,  and  add  water. 
Indigo  sol.  (sulfindigotic  acid).     Slowly  mix  and  stir  5s  indigo  with  25CC  H2SO4 

(or  better  H2S2O7,  fuming  sulfuric  acid)  in  a  beaker  immersed  in  cold 

water.     Cover  the  beaker,  and  after  48  hours  add  500 cc  H20,  stir  and  filter. 
Many  substances  in  sol.  easily  break  up  on  standing,  and  hence  should  be  freshly 

prepared. 
For  acid  radicals  compounds  of  Na  or  K  are  commonly  used,  as  they  are 

soluble. 

vin 


RULES   AND   SUGGESTIONS   FOR   PUPILS. 

Pupils  should  read  .these  rules  carefully,  and  should  refer  to  them  whenever  in 

doubt  on  any  point. 

1.  Each  pupil  should  provide  himself  with  a  towel,  to  keep  his  bench  clean, 
and  any  apron  or  other  clothing  desired  for  protection  in  the  laboratory. 
A  long  linen  duster  or  duck  coat  reaching  to  the  feet  is  the  best  protection. 
Without  something  of  the  sort  clothing  may  be  injured  at  any  moment. 

2.  The  bench  at  which  the  pupil  works  must  be  left  clean  and  dry  after 
every  laboratory  exercise.     Wipe  off  a  ring-stand,  lamp,  or  other  apparatus  on 
which  a  re-agent  has  fallen,  wipe  out  a  p.t.  after  using  it,  and  keep  re-agent 
bottles,  apparatus,  books,  and  lockers  clean. 

3.  Pupils  are  held  responsible  for  apparatus,  and  should  replace  anything 
that  is  lost  or  broken. 

4.  In  experimenting  have  your  apparatus  neatly  arranged  without  artificial 
props,  wedges,  or  uncouth-looking  material.     Have  every  d.t.  and  stopper  fit 
tightly  to  prevent  leakage  of  gas.     If  a  gas  generates  well,  but  does  not  pass 
into  the  rec. ,  there  is  some  leakage,  due  probably  to  loose  bearings. 

5.  In  heating  a  t.t.  on  the  r.s.  hold  the  lamp  in  the  hand,  move  it  slowly, 
and  now  and  then  take  it  away  from  the  tube  for  a  moment,  to  prevent 
melting  and  breaking  the  latter. 

6.  Mixtures  of  solids  should  be  made  on  paper.     Be  careful  not  to  mix 
chemicals  or  re-agents  except  as  directed. 

7.  To  shake  the  contents  of  a  t.t.  cover  its  mouth  with  the  thumb  (Exp.  4, 
Fig.  10),  or  the  hand,  or  a  stopper,  hold  it  away  from  the  bench,  and  shake  it 
vigorously. 

8.  Never  put  down  a  stopper  when  using  a  re-agent  bottle,  but  hold  it 
between  the  first  and  second  fingers  (Exp.  6,  Fig.  11),  and  replace  it  when  you 
put  down  the  bottle.     Do  not  pour  back  any  excess  of  a  re-agent  from  a  t.t.  or 
other  rec.  into  a  re-agent  bottle,  and  do  not  dip  a  stirring  rod  into  a  re-agent 
bottle. 

9.  In  pouring  a  liquid  into  a  t.t.  (or  graduate)  hold  the  latter  on  a  level  with 
the  eye,  and  towards  the  light,  so  as  to  see  any  change.     The  thumb-nail  may 
be  placed  at  the  upper  limit  to  which  it  is  desired  the  liquid  should  reach. 
When  much  heat  is  liberated,  as  when  sulfuric  acid  is  poured  into  water,  a 
tube-holder  should  be  used  ;  paper  folded  several  times  serves  for  this  purpose. 

10.  Pour  only  liquids,  fine  powders,  or  soluble  salts  into  the  sinks,  always 
opening  the  faucet  first  to  let  the    water  run.     Other  solids  should  be  thrown 
into  the  jars.     Great  care  must  be  taken  not  to  clog  the  discharge-pipes. 

11.  Have  flasks  and  tubes  perfectly  dry  on  the  outside  before  applying  heat. 
Tubes  of  thick  glass,  if  they  contain  no  liquid,  should  be  heated  gradually  at 

ix 


TABLE  OF  COMMON  ELEMENTS. 

ARRANGED    ACCORDING    TO    ELECTRO-CHEMICAL    ORDER. 


NAME. 

SYMBOL. 

Oxygen 

0" 

Sulfur 

S",  iv  (vi) 

Nitrogen 

N'",  v-  etc. 

Fluorin 

F',  00 

Chlorin 

Cl',  00 

Bromin 

Br',  CO 

lodin 

T,  (v) 

Phosphorus 

P"',  'V 

Arsenic 

As'",  v 

Chromium 

Cr",  '",  vi 

Boron 

B"' 

Carbon 

CD,  iv 

Antimony 

Sb"',  v 

Silicon 

Si" 

Hydrogen 

H' 

Gold 

Au('),  "' 

Platinum 

Pt("),  IV 

Mercury 

Hg',  " 

Silver 

Ag7 

Copper 

Cu('),  " 

Bismuth 

Bi'",  (v> 

Tin 

Sn",  'v 

Cadmium 

Cd" 

Cobalt 

Co",  ('") 

Nickel 

Ni",  ('") 

Lead 

Pb",  OT, 

Iron 

Fe",  "' 

Zinc 

Zn" 

Manganese 

Mn",  ("') 

Aluminum 

Al'" 

Magnesium 

Mg" 

Calcium 

Ca" 

Strontium 

Sr" 

Barium 

Ba" 

Sodium 

Na' 

Potassium 

K' 

AT.  WT. 

VAPOR  DENSITY. 

STATE, 

16 

16 

G 

32 

32 

S 

14 

14 

G 

19 

G 

35.5 

35.5 

G 

80 

80 

L 

127 

127 

S 

31 

62 

S 

75 

150 

S 

52 

S 

11 

S 

12 

S 

120 

S 

28 

S 

1 

1 

G 

197 

S 

197 

S 

200 

100 

L 

108 

S 

63 

S 

207 

S 

117 

S 

112 

56 

S 

59 

S 

58 

S 

206 

S 

56 

S 

65 

32i 

S 

55 

S 

27 

S 

24 

S 

40 

S 

87 

S- 

137 

S 

23 

S 

39 

S 

A  ( )  indicates  a  rare  valence.     Atomic  weights  are  only  approximate. 

xii 


ABBREVIATIONS. 


Ac.  —  acetate,  C2H802. 

gr.  —  green. 

alk.  —  alkali  or  alkaline. 

insol.  —  insoluble. 

Am.  —  ammonium,  NH4. 

i.t.  —  ignition  tube. 

app.  —  apparatus. 

M.  —  metal  (valence  1). 

b.  —  black. 

.    o.f.  —  oxidizing  flame. 

B.B.  —  before  the  blowpipe. 

Ox.  —  oxalate. 

B.B.C.C.  —  before  the  blowpipe  on 

ppd.  —  precipitated. 

charcoal. 

ppg.  —  precipitating. 

bl.  —  blue. 

ppn.  —  precipitation. 

cc.  —  cubic  centimeters. 

ppt.  —  precipitate. 

cm.  —  centimeters. 

p.t.  —  pneumatic  trough. 

col.  —  color. 

qcm.  —  square  centimeters. 

cone.  —  concentrated. 

re-agt.  —  re-agent. 

cpd.  —  compound. 

rec.  —  receiver. 

cryst.  —  crystalline. 

res.  —  residue. 

Cy.  —  cyanid,  CN. 

r.f.  —  reducing  flame. 

dil.  —  dilute. 

r.s.  —  ring  stand. 

dis.  —  dissolve. 

sat.  —  saturate. 

dist.  —  distinguish. 

sep.  —  separate. 

d.s.  —  deflagrating  spoon. 

si.  —  slight  or  slightly. 

d.t.  —  delivery  tube. 

sol.  —  solution  or  soluble. 

e.d.  —  evaporating  dish. 

sp.  gr.  —  specific  gravity. 

evap.  —  evaporate. 

s.r.  —  stirring  rod. 

ex.  —  excess. 

Tr.  —  tartrate. 

Exp.  —  experiment. 

t.t.  —  test  tube. 

fil.  —  filtrate. 

up.  disp.  —  upward  displacement. 

g.  —  grams. 

v.  —  vide,  see. 

gel.  —  gelatinous. 

vol.  —  volume. 

gen.  —  generator. 

yel.  —  yellow. 

Xlll 


INDEX   TO   EXPERIMENTS. 


1.  Metric  Measurements. 

35.  Oxids  of  Nitrogen. 

69.  Manganese. 

2.  Glass  Manipulation. 

36.  Carbon  Dioxid. 

70.  Zinc. 

3.       "                " 

37.  Chlorin. 

71.  Group  IV. 

4.  Physical  Changes. 

38.  Euchlorin. 

72.  Barium. 

5. 

39.  Bromin. 

73.  Strontium. 

6.  Chemical       " 

40.  lodin. 

74.  Calcium. 

7.  Elements  and  Compounds. 

41.  Sulfur. 

75.  Magnesium. 

8.  Oxygen,  Preparation. 

42.  Hydrogen  Sulfid. 

76.  Group  V. 

9.        "        Combustion. 

43.  Phosphorus. 

77.  Sodium. 

10. 

44.  Arsenic. 

78.  Potassium. 

11.  Nitrogen,  Separation. 

45.  Compounds  of  Boron. 

79.  Ammonium  t 

12.         "         and  Air. 

46.           "           "  Silicon. 

80.  Group  VI. 

13.  Hydrogen  from  Acids. 

47.  Oxidation  and  Reduction. 

81.  Borates. 

14.         "            "    Water. 

48.  Lead. 

82.  Nitrates. 

15.  Carbon,  Preparation. 

49.  Silver. 

83.  Nitrites. 

16.        "        Properties. 

50.  Mercury. 

84.  Chlorates. 

17.  Combustion. 

51.  Group  I. 

85.  Carbonates. 

18.           " 

52.  Mercury. 

86.  Sulfids. 

19.  Positive  and  Negative  Elements. 

53.  Lead. 

87.  Sulfltes. 

20.  Acids,  Bases,  Salts. 

54.  Bismuth. 

88.  Thiosulfates. 

21.  Acid,  Alkaline,  Neutral  Reactions. 

55.  Cadmium. 

89.  Fluorids. 

22.  Soluble  Salts  by  Neutralization. 

56.  Copper. 

90.  Chlorids. 

23.        "          "    from  Metals. 

57.  Group  H,  A. 

91.  Bromids. 

24.        "          "       "    Carbonates,  etc. 

58.  Arsenic. 

92.  lodids. 

25.  Insoluble  Salts  by  Precipitation. 

59.  Tin. 

93.  Acetates. 

26.  Hydrochloric  Acid. 

60.  Antimony. 

94.  Cyanids. 

27.               "                " 

61.  Group  H,B. 

95.  Tartrates. 

28.  Hydrofluoric      «« 

62.  Iron. 

96.  Oxalates. 

29.  Nitric 

63.      " 

97.  Silicates. 

30.  Aqua  Regia. 

64.  Aluminum. 

98.  Ferrocyanids. 

31.  Sulfuric  Acid. 

65.  Chromium. 

99.  Ferricyanids. 

32.  Ammonium  Hydroxid. 

66.  Group  in. 

100.  Sulfates. 

33.  Fixed  Alkalies. 

67.  Cobalt. 

101.  Chromates. 

34.  Oxids  of  Nitrogen. 

68.  Nickel. 

102.  Phosphates. 

xiv 


XT 


1.    METRIC    MEASUREMENTS. 

I.  Length. 

Note  the  length  of  10cm  on  a  metric  ruler,  then  estimate  by  the 
eye  alone  this  length  on  the  cover  of  a  book,  and  on  various  objects, 
verifying  each  result  till  you  can  carry  in  mind  10cm.  Estimate 
the  number  of  inches  it  covers,  and  verify.  In  the  same  way 
experiment  with  lcm.  Measure  the  perpendicular  distance  between 
the  blue  lines  on  a  sheet  of  foolscap  paper.  Measure  the  diameter 
of  the  older  nickel  five-cent  piece.  Make  a  drawing  of  the  fol- 
lowing measurements  on  the  opposite  page :  one  square  decimeter, 
i.e.  10cm  on  a  side ;  lqcm. 

II.  Volume. 

Measure  in  a  graduate  10CC  of  water,  then  pour  it  into  a  t.t. 
Note,  without  marking,  what  proportion  of  the  t.t.  is  filled.  Make 
a  drawing  of  it  on  the  opposite  page.  Pour  out  the  water,  then 
pour  into  the  t.t.  as  near  the  same  volume  as  possible,  estimating 
by  the  eye  alone.  Verify  the  result  by  pouring  the  water  into  the 
graduate.  Kepeat  this  till  you  can  estimate  quite  accurately.  Try 
it  with  a  t.t.  of  another  size.  Estimate  lcc  of  the  liquid  in  the 
same  way.  Draw  a  figure  of  a  cube  lcm  on  a  side. 

In  future  experiments  estimate  volumes,  without  measuring,  unless 
special  accuracy  is  required. 

III.  Weight. 

Balance  a  piece  of  paper  on  each  pan  of  a  pair  of  scales.  On 
one  pan  put  a  10g  weight  and  balance  this  with  fine  salt  or  sugar. 
Note  with  the  eye  the  quantity  of  the  substance,  then  remove  it. 
Now  estimate  a  like  quantity  and  verify  by  weighing  it.  Repeat 
the  experiment  several  times.  Weigh  1  or  2g  and  estimate  as 
before.  See  if  lg  can  be  piled  on  a  one-cent  coin.  Weigh  one  of 
the  old  nickel  five-cent  pieces.  In  subsequent  experiments  estimate 
quantity  of  solids,  unless  accuracy  is  desired. 

Supplementary.  —  Commit  to  memory  the  metric  tables  for  length,  volume 
and  weight  (v.  Physics).  How  many  cc  in  a  liter  ?  How  many  grams  should  a 
liter  of  water  weigh  ?  10CC  of  water  ?  Hg  weighs  13.6  times  as  much  as  water. 
What  will  5|cc  of  Hg  weigh  ?  A  rectangular  block  of  marble  is  3  X  4  X  2cm 
and  has  sp.  gr.  2.5.  What  does  it  weigh  in  grams  ? 


2.    GLASS    MANIPULATION. 


I.  Ignition  Tubes. 

Take  a  piece  of  ignition  tubing  20  or  25cm  long, 
hold  it  steadily  in  a  Bunsen  flame  just  above  the  inner 
greenish  cone  (Fig.  1),  and  rotate  it.     When  it  begins 
to  soften  draw  it  out  slightly  (Fig.  2,  a)  and  raise  it 
a  little  in  the  flame.     Do  not  pull  or  twist  the  glass 
but  let  the  heat  gradually  separate  it,  so  as  not  to 
have  long  threads  attached.    The  ends  may  be  rounded 
(Fig.  2,  b)  by  holding  in  the  edge  of  the  flame  (Fig.  3). 
Finally  anneal  the  glass  by  closing  the  lower  open- 
ings of  the  lamp  and  holding  the  heated  end 
in  the  flame  to  cover  it  with  soot,  then  letting 
Fi  it  cool  gradually  without  touching  any  object. 

Unless  great  care  is  taken  in  this,  the  glass 

will  break  when  next  put  into  the  flame.     Save  the  tubes  for  sub- 
sequent experiments. 


II.  Stirring  Rod. 


Weld  the  ends  of  a  piece  of  glass  tubing  about 
locm  long  and  £  or  ij-cm  in  diameter  by  holding  each 
end  successively  in  a  Bunsen  flame  above  the  green 
cone  (Fig.  3),  and  rotating  till  the  openings  are 
sealed.  Use  care  in  cooling  as  before. 


Fig.  3. 


Supplementary.  —  Bulb  Tubes.     Draw  out  a  piece 
of  tubing  as  in  1,  then  melt  the  closed  ends  by  holding 
and  rotating  as  in  Fig.  3.     When  the  glass  is  sufficiently 
Fig.  4.  softened,  blow  moderately  into  the  open  end,  repeating 

the  operation  till  the  tube  assumes  the  desired  shape  (Fig.  4). 


3.    GLASS    MANIPULATION. 

III.  Connecting  Tubes, 

Use  an  ordinary  gas  flame  (or  a  fish-tail  attachment  to  a  Bunsen 
burner)  for  bending  glass,  as  the  Bunsen 
flame  is  too  hot.  Turn  down  the  gas  till 
the  flame  is  about  5cm  across,  then  bend 
each  of  3  pieces  of  tubing,  16cm  long,  in  the 
middle  and  at  right  angles,  by  letting  the 
glass  rest  lightly  in  the  fingers  of  both 
hands  and  holding  it  lengthwise  of  the  flame 
and  just  above  the  dark  part  (Fig.  5).  Ko- 
tate  it  slowly  and  hold  very  steadily.  When 
it  begins  to  soften  take  it  quickly  from  the 
flame  and  —  holding  it  between  the  eye  and 
a  window  frame  —  bend  it  at  right  angles. 
If  it  does  not  bend  easily,  heat  it  again.  Bend  also  one  piece  of 
tubing  (50cm  long),  5  or  6cm  from  one  end.  Kound  the  sharp 
corners  of  each  by  holding  the  tip  ends  of  the  tubes  in  the  edge  of 
a  Bunsen  flame  for  a  minute  (Fig.  3).  Do  not  let  any  part  of  the 
heated  glass  touch  any  object  and  avoid  wiping  off  the  soot  till  the 
glass  is  cool  enough  to  handle,  when  it  should  be  cleaned. 

IV.  Delivery  Tubes, 

Examine  the  angles  (all  obtuse)  and  the  relative  lengths  of  the 

parts  in  Fig.  6  and  in  a  model, 
noting  that  the  bends  a  and  c  are 
very  near  the  ends,  and  a  and  b 
are  close  together.  Do  this  work 
very  carefully.  Use  a  piece  of 
glass  tubing  50cm  long,  holding  it 
as  before.  Make  the  bends  in  the 
order  a,  b,  c.  Hold  the  glass  con- 
stantly  in  the  flame,  turning  it 
6  occasionally  to  heat  both  sides. 

When  it  yields  remove  and  bend  it 
out  of  the  flame.  To  make  the  bends  at  b  and  c,  turn  the  glass 
quickly  and  —  closing  one  eye  —  sight  along  the  tube  so  as  to 
have  all  parts  lie  in  the  same  plane.  Round  the  sharp  edges  1 
and  2  in  the  flame,  as  before,  and  cool  with  care.  Show  all  results 
to  the  instructor. 

V.  Perforating  Corks. 

Fit  a  cork  to  a  t.t.,  remove  it  and  with  a  round  file  bore  a  hole 
in  it  —  holding  the  cork  in  the  left  hand  and  pressing  the  end  of 
the  file  against  its  larger  surface.  Observe  constantly  during  the 
operation  whether  the  perforation  is  perpendicular  to  the  surface  of 
the  cork.  The  orifice  must  be  perfectly  circular  and  a  little  smaller 
than  the  tube  it  is  to  receive.  When  completed,  adjust  to  the  d.t. 
and  t.t.  Detach  the  stopper  from  the  t.t.,  not  from  the  d.t. 


4.    PHYSICAL    CHANGES. 


Fig.  7. 


Solution. 

See  whether  crystals  of  granulated  sugar,  C12(H20)U,  can  be 
crushed.      Put  into  a  t.t.   5g  or  more  of  the 
sugar,  just  cover  it  with  water,  H20,  and  boil 
in  a  Bunsen    flame  for  a  minute,  using  a  t.t. 
holder  of  wood,  metal,  or  paper  (Fig.  7),  till 
the  sugar  dissolves.      Cool  it  by  holding  the 
tube  under  a  jet  of  water,  and  when  cool  taste 
a  drop  of  the  liquid.     Have  the  sugar  particles 
been   divided   by   dissolving?      How   do   you 
know?     Arrange  a  filter  paper  (Fig.  8)  and 
filter  the  sol.,  using  a  filter  stand  and  collect- 
ing the  filtrate  in  another  t.t. 
(Fig.   9).      Touch  a  drop  of 
the  filtrate  to  the  tongue  with 
a   stirring   rod    (s.r.).     Note 
whether  the  sugar  has  gone 
through     the     filter     paper. 
Divide  the  liquid  into  two  parts.    Save  one  for 
Exp.  6,  and  dilute  the  other  with  an  equal  vol. 
of  H20  ;  then  cover  the  t.t.  with  the  thumb  or 
hand,  invert  it  (Fig.  10)  and,  holding  it  away 
from  the  table,  shake  the  contents  vigorously. 
Taste  a  drop  of  the  sol.     Note  whether  the 
Fig  9  sugar  particles  have  been  further,  divided. 

Supplementary,  —  Read  very  carefully  Rule  14  and  the  Model  for  Taking 
Notes,  (a)  Dis.  a  little  CuCl2  or  Cu(NO3)2  in  water, 
boiling  as  before,  and  filter  but  do  not  taste  the  sol. 
(b)  Dis.  also  a  little  NaCl,  filter  and  taste  the  filtrate. 
Evaporate.  Do  substances  in  sol.  pass  through  a 
filter  paper  ?  Many  substances  like  SiO2  and  BaS  0* 
are  not  sol.  in  water  or  acids,  others,  like  Zn,  Cu, 
etc.,  are  sol.  hi  acids  only,  (c)  Heat  a  platinum 
wire  in  a  Bunsen  flame.  Note  if  it  undergoes 
change. 


Fig.  8. 


Fig.  10. 


Terms:  Physical  division,  physical  solution,  insoluble,  dilution,  molecule, 
evaporation,  properties,  filtrate,  residue. 


5.    PHYSICAL    CHANGES. 

Solution  and  Crystallization. 

1.  Fill  an  e.d.  f  full  of  water,  heat  it,  and  add  small  pieces  of 
alum  until  the  liquid  becomes  thick.    Replace  the  water  lost  by  evap- 
oration.    Now  put  in  a  narrow  piece  of  cotton  cloth  so  that  it  lies 
in  the  liquid  but  does  not  touch  the  bottom  of  the  dish,  and  set  the 
latter  aside  to  cool.     Observe  occasionally,   meantime  doing  the 
following  : 

2.  Cautiously  boil  about  5g  copper  sulfate  in  5CC  H20  in  a  t.t. 
until  it  is  dissolved.     Then  place  the  t.t.  in  an  oblique  position 
and  let  the  liquid  cool.     If  necessary,  leave  till  the  next  laboratory 
hour.     Note  the  formation  of  crystals  in  1  and  2,  and  observe  their 
form,  color,  luster,  angles,  etc.     Are  these  illustrations  of  physical 
or  of  chemical  changes,  and  why  ?     Trace  each  step  in  the  process. 
Which  seems  more  soluble,  alum  or  sulfate  of  copper  ?     Are  they 
more  soluble  in  hot  or  in  cold  water  ? 

3.  Put  a  few  crystals  of  copper  sulfate  into  an  i.t.  or  small  t.t. 
and  slowly  heat.     Observe  the  sides  of  the  tube  and  any  change  of 
color,  luster,  hardness,  and  form  in  the  crystals.     Explain.     When 
the  tube  is  cool  add  a  drop  of  water. 

4.  Experiment  in  the  same  way  with  some  of  the  crystals  of 
alum,  tasting  the  powder  obtained  by  heating. 

5.  Put  a  crystal  of  sodium  sulfate  and  a  small  piece  of  calcium 
chlorid  on  separate  pieces  of  paper  and  leave  them  in  the  locker 
exposed  to  the  air  till  the  next  exercise.     Describe  the  result  with 
explanation. 

Supplementary.  —  (a)  Put  into  an  e.d.  as  much  powdered  S  as  will  stay  on 
the  point  of  a  very  small  knife  blade.  Cover  it  with  a  very  little  C  S2  (keep  the 
flame  at  a  distance  from  this  substance)  so  as  to  dis.  the  S,  let  it  evaporate  in  a 
draft  of  air,  then  watch  closely  as  the  C  S2  evaporates.  Describe  and  explain  the 
phenomena.  Put  a  drop  of  this  sol.  on  a  microscopic  slide  and  watch  it  closely 
under  the  microscope  as  the  CS2  evaporates,  (b)  Dissolve  and  re-crystallize 
Na2SO4.  (c)  Mix  sols,  of  alum  and  CuSO4  and  try  to  crystallize  the  two 
substances  together.  Are  the  above  salts  soluble  or  insoluble  ? 

Terms:  Crystal,  amorphous  substance,  mother  liquor,  saturation,  super- 
saturation,  water  of  crystallization,  deliquescent,  efflorescent,  luster. 


6.    CHEMICAL,    CHANGES. 

I.  Sulfuric  Acid  and  Sugar. 

To  the  sol.  saved  from  Exp.  4  slowly  add  sulf uric  acid,  H2S  04, 
in  a  small  stream,  holding  the  tube  with  a  t.t. 
holder,  and  the  bottle  as  in  Fig.  11  (read  Rule 
9),  till  the  substance  changes  color.  Add  a  little 
more  acid,  and  if  the  sugar  solution  is  strong 
enough  it  will  cause  the  substance  to  swell  and 
run  over  the  tube.  Observe  the  color,  odor,  and 
temperature,  but  do  not  taste  it.  Does  it  appear 
Fig.  11.  to  be  a  solid  or  a  liquid  ?  Sugar  is  a  compound 

of  C  and  H20.  H2S04  has  great  affinity  for 

water.     From  these  facts  explain  the  phenomena.     Clean  the  tube 

with  water,  using  a  brush  if  necessary. 

II.  Heat  and  Sugar. 

See  whether  heat  will  break  up  sugar,  by  dipping  a  short  piece 
of  glass  tubing  moistened  with  water  into  a  little  sugar  and 
holding  it  in  a  Bunsen  flame.  Describe  all  you  see,  note  the  odor, 
and  state  your  conclusions.  What  produced  the  chemical  change  ? 

III.  Combustion  of  Wood. 

Hold  a  small  stick  in  a  flame.  State  whether  the  changes 
observed  are  chemical,  or  physical,  with  reasons. 

IV.  Changes  in  Solutions. 

Add  a  little  hydrogen  chlorid,  HC1,  to  5CC  Pb(N08)a  sol.  The 
hydrogen  chlorid  and  the  lead  nitrate  have  become  lead  chlorid 
and  hydrogen  nitrate.  The  former  product  is  insoluble  and  is 
therefore  thrown  down  (precipitated).  To  5CC  of  CuCl2  sol.  add  a 
little  N  H40  H  —  ammonium  hydroxid  —  and  notice  any  evidence  of 
change. 

Supplementary.  — (a)  To  5CC  of  HgCl2  sol.  add  a  few  drops  of  KI  sol. 
(b)  Add  a  few  drops  of  KI  sol.  to  5CC  of  Pb(NO3)2  sol.  (c)  On  a  few  bits  of  Cu 
in  an  e.d.  pour  a  few  drops  of  nitric  acid,  HNOa.  Describe  all  you  see.  Are 
these  chemical,  or  physical  changes  ?  Why  ? 

Terms :  Combustion,   chemical  solution,  affinity,   precipitation,  chemical 


7.    ELEMENTS    AND    COMPOUNDS. 


Fig.  12. 


Synthesis. 

Fill  an  i.t.  (from  Exp.  2)  not  over  -j-  full  of  an  intimate 
mixture  of  one  part  by  weight  of  S  (finely  pow- 
dered brimstone,  or  flowers  of  S)  with  two  parts 
of  fine  Cu  filings.  Observe  that  the  two  elements 
are  entirely  distinct,  and  note  the  color  and 
luster  of  each.  Now  heat  the  tube  very  slowly 
for  a  minute  (moving  it  alternately  out  of  the 
flame  and  into  it,  so  as  not  to  break  the  glass) 
then  heat  very  strongly,  'the  upper  part  first 
(Fig.  12).  Watch  the  contents  of  the  tube  for 
evidence  of  a  chemical  change.  What  is  the 
evidence  ?  When  this  change  has  taken  place  throughout  the 
whole  mass  let  the  tube  cool  for  a  minute,  then  heat  an  instant, 
break  the  -tube  with  a  jet  of  water,  and  examine  the  substance. 
Note  whether  it  resembles  Cu  or  S  in  color  or  luster.  Describe 
fully  what  you  saw,  state  what  is  supposed  to  have  taken  place, 
and  give  an  equation  to  express  it. 

Supplementary.  —  (a)  Mix  Fe  filings  and  S  (in  about  the  same  proportion  as 
Cu  and  S),  try  to  separate  the  Fe  with  a  magnet  and  the  S  with  C  S2  from  a 
part,  then  heat  the  other  part  in  an  i.t.  Test  the  product  with  magnet  and 
CS2 ;  also  by  adding  a  little  H2O  and  then  HC1  in  an  e.d.  An  offensive  gas  is 
liberated  which  either  element  alone  would  not  give  if  similarly  treated. 
Describe  fully  with  equations,  (b)  Light  a  match,  and  as  it  burns  watch  the 
colors  of  the  flame  and  see  if  there  is  any  evidence  of  a  product  being  formed. 
The  match  contains  the  elements  P,  S,  and  C,  which  combine  with  the  element 
O  in  the  air  to  form  compounds  called  oxids  of  P,  S,  and  C  (v.  Exp.  9). 
(c)  Burn  a  piece  of  charcoal  and  observe.  The  products  are  for  the  most  part 
invisible  gases,  (d)  Heat  in  an  i.t.  a  little  granular  pyrite,  FeS2,  and  finally 
test  the  residue  with  a  magnet.  • 


Terms:    Synthesis,   sulfid,   oxid,   binary  compound,  element,  gas,  luster, 
residue. 


Fig.  13. 


8.    PREPARATION    OF    OXYGEN. 

Fill  4  or  5  wide-mouthed  bottles  —  recs.  —  with  water,  invert 

them  on  the  shelf  of  a  p.t. 
in  which  the  water  is  3  or 
4cm  above  the  shelf.  Mix  on 
a  paper  5  or  10g  KC10a 
(not  pulverized)  and  3  or  4« 
of  powdered  Mn02.  Put 
the  mixture  into  a  large  dry 
t.t.  which  should  not  be  over 
•J-  full.  Adjust  a  stopper  and 
d.t.  and  hang  the  app.  on  a 
r.s.  (Fig.  13).  Direct  a 

Bunsen  flame  against  the  t.t.,  holding  the  lamp  and  slowly  moving 
it.  Avoid  heating  too  long  in  one  place  (take  it  away  from  the 
tube  occasionally  for  a  few  seconds),  or  the  tube  will  melt.  Watch 
the  bubbles  in  the  d.t.,  collect  the  escaping  gas  in  the  recs.,  and 
notice  the  bubbles  as  they  burst,  and  whether  the  gas 
has  color.  Explain,  and  after  a  time  observe  again. 
Is  there  evidence  of  a  gas,  or  a  solid,  or  both  ?  As 
soon  as  the  flame  is  taken  away  remove  the  d.t.  from  the 
trough  to  prevent  the  water  drawing  back  and  break- 
ing the  tube.  Why  is  there  this  back  action  ?  Let 
the  recs.  remain  on  the  shelf  till  wanted,  or,  if  taken 
out,  keep  them  covered  with  glass  plates  (Fig.  14). 
After  doing  Exp.  9  clean  the  t.t.  by  covering  the  residue  with 
water,  closing  the  mouth  of  the  tube  with  the  thumb  or  hand,  and 
shaking  the  contents  vigorously,  holding  it  away  from  the  table. 

Supplementary.  —  Does  the  O  occupy  more,  or  less,  volume  than  the  factors 
from  which  it  was  obtained  ?  Why  ?  Would  it  weigh  more,  or  less  ?  Why  ? 
The  MnO2  takes  no  part  in  the  reaction,  but  is  used  to  distribute  and  equalize 
the  heat  and  lower  the  temperature  of  dissociation.  Name  all  the  substances 
in  the  t.t.  at  the  end  of  the  exp. 


Fig.  14. 


Terms :  Factors,  products,  dissociation. 


9.    COMBUSTION  IN  OXYGEN. 

1.  Put  a  burning  splinter  into  a  rec.  of  0  for  an  instant,  note 
the  color  and  vigor  of  the  flame,  then  remove,  blow  out  the  flame 
and  put  in  the  glowing  stick.     Repeat  till  there  is  no  effect.     State 
accurately  everything  you  saw  and  heard.     Wood  consists  largely 
of  C.     Explain  the  combustion  and  write  an  equation  for  it.     Test 
the  product  by  adding  4  or  5CC  of  lime  water,  Ca(OH)2  sol.;  shake 
it  well  and  notice  the  effect. 

2.  Make  a  d.s.  by  hollowing  out  the  end  of  a  crayon,  or  electric 

light  carbon,  and  attaching  a  Cu  wire.  Put  into  it  a 
bit  of  S,  hold  the  whole  in  a  flame  till  the  S  burns, 
then  lower  it  into  a  rec.  of  0  (Fig.  15).  Notice  the 
color  and  vigor  of  the  flame,  and  the  color  and  state  of 
the  product,  explain  what  you  see  and  write  the  equa- 
tion. Name  the  product  and  test  it  by  cautiously 
noting  the  odor,  and  also  by  putting  a  drop  of  K2Cr207 
sol.  on  paper  and  holding  it  in  the  gas,  noting  any 
Fig- 15-  change  of  color. 

3.  Put  into  an  e.d.  with  a  pair  of  forceps  (don't  handle  it) 
a  piece  of  P,  half  as  large  as  a  pea.     Dry  it  by  rolling  it  lightly  on 
paper,  then  put  it  into  a  d.s.     Heat  for  an  instant  the  end  of  a 
wire  or  file,  touch  the  P  with  it  and  lower  the  spoon  at  once  into  a 
rec.  of  0.     Observe  the  color  of  the  flame  and  of  the  product. 
Describe,  also  write  the  equations.     When  combustion  stops  burn 
every  bit  of  the  P  by  holding  the  d.s.  in  a  flame.     Add  a  few  cc  of 
H20  to  the  rec.,  shake  it  well  and  drop  in  a  piece  of  blue  litmus 
paper. 

Supplementary.  —  What  became  of  the  0  in  the  above  cases  ?  Would  the 
product  in  each  case  weigh  more  or  less  than  the  C,  S,  P  ?  How  do  you 
know  ?  (a)  Cover  the  bottom  of  a  rec.  of  O  with  sand  or  H20  1  or  2cm  deep. 
With  forceps  hold  for  an  instant  in  a  flame  one  end  of  a  picture-cord  wire  5  or 
10cm  long,  then  dip  it  into  a  bit  of  powdered  S.  Hold  it  again  in  the  flame  till 
the  S  burns,  then  thrust  it  into  the  rec.  of  O.  If  the  Fe  does  not  burn  try  it 
again,  or  repeat  with  another  rec.  (have  but  little  S  on  the  wire).  Describe  the 
combustion  and  the  product,  and  give  the  equation,  (b)  With  forceps  hold  in 
the  flame  a  piece  of  Mg  ribbon  till  it  begins  to  burn,  then  instantly  thrust  it  into 
a  rec.  of  O.  (c)  Try  Zn  tipped  with  S. 

Terms :  Supporter  of  combustion,  combustible,  kindling  point. 


1O.    OXYGEN. 


Fig.  16. 


I.  Oxygen  from  Oxids. 

Heat  strongly  1  or  2g  of  HgO  in  a  t.t. 
or  i.t.  and  thrust  a  glowing  splinter  into 
the  tube  while  still  holding  it  in  the 
flame  (Fig.  16).  Note  the  color  of  the 
HgO  while  it  is  being  heated,  observe  the 
sides  of  the  tube,  and  finally  pour  out  and 
carefully  examine  the  contents.  Explain, 
and  give  the  reaction.  Save  the  residue. 


II.  Oxygen  from  Nitrates. 

Put  into  a  t.t.  about  1«  of  Pb  (N08)2, 

heat  it  and  test  the  gas  as  before.  Note  any  snapping,  the  color  of 
the  fumes,  which  are  N  02  and  0  (the  O  being  colorless),  and  the 
color  of  the  residue,  PbO.  Also  write  the  equation. 

III.  Oxygen  from  Chlorates. 

Try  to  obtain  oxygen  in  the  same  way  by  heating  a  few  crystals 
of  K  C103.     Test  as  before,  and  write  full  notes. 

Supplementary.  —  What  3  classes  of  substances  have  you  found  which  yield 
O  ?  From  which  is  the  oxygen  obtained  most  easily  ?  N2O  will  also  support 
combustion  of  C,  S,  P,  but  not  as  readily  as  pure  O.  Heat  and  test :  (a) 
(b)  NaNO3. 


Terms:   Oxid,  chlorate,  chlorid,  nitrate,  residue. 


11.     SEPARATION  OF  NITROGEN. 

Fill  a  p.t.  with  water  3  or  4CC  above  the  shelf.  Prepare  a  d.s. 
with  a  wire  bent  sharply  5  or  6cm  from  the 
crayon.  Pass  the  wire  through  the  orifice  in 
the  shelf  so  that  it  will  reach  half  way  up  an 
inverted  rec.,  fasten  it  there  (so  as  to  be  easily 
removable)  with  the  mouth  of  the  rec.  under 
water  (Fig.  17).  When  adjusted  remove  the 
rec.,  leaving  the  wire.  Using  forceps  and  e.d. 
put  a  piece  of  P  (the  size  of  half  a  pea)  into 
Fis- 17-  the  spoon.  Touch  it  with  a  warm  (but  not  too 

hot)  wire  or  file  handle,  and  instantly  invert  the  rec.  over  it  as  be- 
fore, pressing  the  latter  down  and  holding  it  steadily  with  the  hand 
till  combustion  ceases.  Was  there  any  escape  of  gas  ?  Before  re- 
moving the  d.s.  be  sure  the  combustion  has  stopped,  and  let  no  air 
enter.  Compare  the  combustion  and  the  product  with  the  same  in 
the  oxygen  exp.  Describe  fully  with  equation.  Finally  remove 
the  crayon  without  admitting  air  or  disturbing  the  rec.  Burn  any 
remaining  P  in  a  flame  and  leave  the  rec.  till  the  gas  becomes  toler- 
ably clear,  then  remove  with  a  glass  plate,  turning  the  rec.  right 
side  up  and  keeping  the  water  in  the  bottom.  Set  this  aside  for 
Exp.  12. 

Supplementary.  — (a)  Try  to  separate  the  N  in  air  with  S  in  a  d.s.,  setting 
the  S  on  fire  by  holding  a  flame  over  the  adjusted  spoon,  (b)  Try  paper  or 
charcoal.  What  elements  do  these  exps.  show  to  exist  in  the.  air  ?  N  may  also 
be  separated  by  forcing  air  over  red  hot  Cu,  which  forms  CuO.  It  may  be 
obtained  from  compounds,  such  as  nitrates  and  ammonia. 


12.    NITROGEN  AND  AIR. 

I.  Properties  of  N. 

(1)  Put  a  burning  stick  into  the  rec.  of  N  (Exp.  11),  sliding 
along  the  glass  cover  enough  to  admit  it.  Note  the  effect  on  the 
stick  and  on  the  gas.  Try  it  with  a  glowing  stick.  Is  the  spark 
rekindled,  or  extinguished  ?  (2)  See  whether  the  P,  S,  and  C  on 
the  end  of  a  match  will  burn  in  the  gas.  Is  there  any  equation  ? 
Why  ?  Is  N  a  combustible  ?  A  supporter  of  combustion  ?  (3)  Test 
the  liquid  with  blue  litmus  paper.  Describe  and  explain. 

II,  Composition  of  Air. 

Measure  accurately  the  water  in  the  rec.  of  N  by  pouring  it  into 
a  graduate  and  recording  the  volume  in  cc.  Then  measure  the 
total  capacity  of  the  rec.  in  the  same  way,  and  compute  the  percentage 
of  0  and  of  N  (by  volume)  in  the  air,  giving  the  computation  and 
remembering  that  the  first  vol.  of  water  represents  the  vol.  of  0 
burned.  If  any  air  was  forced  out  in  Exp.  11,  will  the  per  cent 
of  0  found  be  too  large  or  too  small  ?  Explain. 

Supplementary.  —  Compare  the  properties  of  N  with  those  of  0.  Air  con- 
tains also  C  02  (tested  for  by  Exp.  36)  and  H2O  (shown  by  setting  a  pitcher  of 
cold  water  in  a  warm  room).  Make  tests  for  each  and  explain.  From  the  per- 
centage of  N  there  must  be  subtracted  about  1%  of  the  recently  discovered  ele- 
ment argon,  A,  a  gas  more  inert  than  N. 

Terms:  Inert  substance,  percentage  by  volume  and  by  weight,  acid,  litmus 
paper. 


13.    HYDROGEN  FROM  ACIDS. 


Fig.  19. 


I.  Preparation. 

Fill  4  or  5  recs.  with  water  and  invert  in  a 
p.t.,  then  put  into  the  gen.  (Fig.  18)  (or  use 
the  same  app.  as  for  making  0)  8  or  10g  granu- 
lated Zn,  cover  with  H20  and  add  5CC  of  HC1 
through  the  thistle  tube.  Have  the  bearings 
perfectly  tight,  and,  without  applying  heat, 
collect  the  gas  like  0.  Observe  and  describe 
the  action  and  note  any  heat.  If  action  stops 
add  more  H  Cl.  Leave  the  recs.  of  gas  in  the  ^s-  is. 

p.t.  till  wanted  in  II  (or  if  removed  keep  them  inverted,  Fig.  19). 
Has  the  gas  any  color  ?     Why  ?     Clean  the  app.  and 
save  the  Zn. 

II.  Tests. 

(1)  Lift  a  small  rec.  of  H,  hold  it  inverted,  and 
thrust  a  burning  stick  into  the  gas.  Note  any  explo- 
sion and  whether  the  gas  or  splinter  burns.  (2)  Try 
it  with  another  rec.  and  then  cautiously  look  into  the 
open  mouth  of  the  latter,  noting  the  colors  of  flame.  Explain  fully 
the  explosion,  combustion,  etc.,  with  equation.  Note  the  (3)  color 
and  (4)  odor  of  (the  impure)  H.  (5)  Collect  by  up.  disp.  a  t.t.  of 
H,  and  test  by  putting  it  mouth  to  mouth  with  a  t.t.  of  air  and  then 
bringing  the  two  open  tubes  successively  to  a  flame. 

Supplementary.  —  (a)  Put  2  or  3  small  pieces  of  Zn  into  a  t.t.  (use  a  t.t. 
holder),  cover  it  with  water  and  add  a  little  H2S04.  Notice  the  action,  test  the 
combustibility  of  the  gas,  and  write  the  equations,  (b)  Put  into  a 
t.t.  a  few  Fe  filings,  add  H2O  and  HC1.  Test  the  gas  as  before, 
(c)  Try  Fe  and  H2SO4.  Make  a  complete  record  of  all  work. 
From  what  class  of  substances  has  H  been  obtained,  and  how  ? 
Is  H  a  combustible  ?  A  supporter  ?  (d)  Try  the  action  of  Zn  and 
H2S  O4,  without  H2O,  cautiously  noting  the  odor,  (e)  Pass  H  into 
euchlorin  (Exp.  38).  (f)  Fill  a  rec.  half  full  of  water,  invert  it  in 
a  p.t.,  letting  air  fill  the  upper  half.  Now  fill  the  rest  with  H  from 
a  gen.,  then  bring  the  mouth  of  the  rec.  to  a  flame,  (g)  Make  a 
philosopher's  lamp  (Fig.  20),  but  before  lighting  the  hydrogen,  test 
the  gas  by  collecting  a  t.t.  full  by  upward  displacement  and  bring- 
ing it  to  a  flame.  If  a  sharp  sound  ensues  there  is  danger,  as  the 
gen.  contains  air.  If  only  a  low  muffled  sound,  the  gas  may  be  lighted.  Lower 
a  larger  open  glass  tube  over  the  flame.  Other  flames  give  the  same  result. 

Terms :   Upward  and  downward  displacement,  philosopher's  lamp,  singing 
flame. 


Fig.  20. 


14.    HYDROGEN  FROM  WATER. 

I,  Action  of  Na  on  H20. 

(1)  Put  into  a  clean  rec.  15  or  20CC  of  H2O.  Have  a  cover  of 
paper  or  cardboard,  not  glass.  Observe  the  color  and 
luster  of  freshly  cut  Na;  take  a  small  piece  from 
the  naphtha  in  which  it  is  kept  (using  forceps  and 
dry  e.d.),  drop  it  into  the  rec.,  and  cover  the  latter  at 
once  (Fig.  21).  Describe  the  action,  note  any  fumes 
or  gas  (try  to  ignite  it),  and  write  equations.  When 
action  stops  take  off  the  cover  and  bring  the  fumes 
near  a  Bunsen  flame,  or  hold  the  lower  openings  of 
the  burner  close  to  the  mouth  of  the  rec.  and  notice  the  color  im- 
parted to  the  flame.  This  is  the  flame  test  for  Na  and  its  cpds. 
Are  the  fumes  solid  or  gaseous,  and  what  becomes  of  them  ? 
(2)  Hold  a  piece  of  moist  red  litmus  paper  in  the  fumes,  also  put 
one  into  the  liquid.  Test  the  liquid  by  adding  a  little  to  these 
sols.:  (3)  FeCl3;  (4)FeS04;  (5)  A1C18. 

(6)  Try  the  action  of  Na  on  hot  H20  by  boiling  a  little  H2O  in  a 
t.t.  and  pouring  it  into  a  rec.,  then  dropping  a  piece  of  Na  on  it  and 
covering  it  at  once.  Note  all  the  phenomena  and  write  equations 
for  :  (a)  the  action  of  Na  on  H20  ;  (b)  the  combustion  of  H,  and 
(c)  Na  ;  (d)  the  sol.  of  Na20. 

II,  Action  of  K  on  H20. 

Perform  the  exp.  as  above,  using  K  and  cold  H20,  and  making 
similar  observations,  notes,  and  tests,  including  flame  tests. 

Supplementary.  —  Which  has  greater  affinity  for  H20,  Na  or  K  ?  (a)  Col- 
lect H  by  putting  a  small  piece  of  Na  in  a  wire  cage  and  quickly  thrust  it  under 
an  inverted  t.t.  full  of  H2O  in  a  p.t.  Test  the  gas.  What  proportion  of  H  in 
water  is  replaced  by  K  or  Na  ?  Are  the  metals  heavier  or  lighter  than  H2O  ? 
(a)  Moisten  a  piece  of  paper,  put  it  into  a  rec.  and  drop  on  the  moist  paper  a 
bit  of  Na  and  cover  it.  When  action  stops  try  to  light  the  fumes  by  bringing  a 
Bunsen  flame  to  the  mouth  of  the  rec.  (b)  Try  the  same  with  K. 


15.    AMORPHOUS  CARBON. 

I.  Carbon  from  Wood. 

Put  2  or  3  small,  thin  pieces  of  wood  into  a  small  Hessian  cruci- 
ble and  cover  them  with  sand  (Fig.  22).  Apply  a 
Bunsen  flame  for  half  an  hour,  or  until  gases 
cease  to  come  off  (meanwhile  do  II,  III,  and 
Exp.  16).  Notice  any  gases  rising  and  try  to 
kindle  them.  Observe  the  color  and  odor.  Finally 
remove  the  carbon  with  forceps  and  save  the  sand. 
Examine  the  carbon  as  to  color,  weight,  volume, 
porosity,  and  brittleness  (compare  with  the  original 
22  wood).  See  whether  it  burns  with  flame  or  only 

glows,  on  igniting  it  in  a  flame. 

II.  Carbon  from  Candle,  Oil,  Gas. 

Hold  a  short  piece  of  white  crayon,  or  of  glass  tubing,  in  the 
flame  of  a  Bunsen  burner,  with  the  lower  openings  closed,  then 
open  the  orifices  and  try  to  burn  off  the  deposit.  Try  to  collect  C 
from  a  candle  flame  and  from  that  of  a  kerosene  lamp  in  the  same 
way.  The  candle,  oil,  and  gas  consist  mainly  of  cpds.  of  C  and  H. 
Which  seems  to  burn  at  the  lower  temperature,  C  or  H  ? 

III.  Carbon  from  Sugar,  Starch. 

Heat  in  a  narrow  tube  a  very  little  sugar,  also  starch.  State 
what  you  see  and  conclude. 

Supplementary.  —  Gases  burn  with  flame.  Solids  glow.  What  has  the 
destructive  distillation  of  wood  in  I.  done  ?  Cpds.  of  C  and  H  (called  hydro- 
carbons) are  solid,  liquid,  or  gaseous,  (a)  Try  to  obtain  carbon  in  any  other 
way,  (b)  Hold  a  piece  of  charcoal  in  water  for  a  minute,  (c)  Weigh  a  piece 
of  wood,  then  distil  it,  and  finally  weigh  the  product,  (d)  Put  some  small 
pieces  of  wood  into  an  i.t.,  attach  a  d.t.  and  heat.  Collect  the  gas  (Fig.  13). 
(e)  Test  the  gas. 

Terms :  Amorphous,  crystalline,  dimorphous,  trimorphous,  porosity,  specific 
gravity. 


16.  PROPERTIES  OF  CHARCOAL,, 

I.  Carbon  a  Reducing  Agent, 

Fill  an  i.t.  not  over  £  full  of  an  intimate  mixture  of  CuO  and  C 
(powdered  charcoal),  about  7  parts  CuO  to  1  part  C  by  weight. 
Heat  it  very  cautiously  at  first,  then  strongly  till  you  see  evidence 
of  a  chemical  change.  What  is  the  evidence  ?  What  caused  the 
mixture  to  rise?  After  the  action  stops  is  there  any  change  in 
color  ?  When  sure  that  no  more  action  will  ensue,  cool  it  for  a 
minute  and  pour  the  contents  into  a  dry  e.d.  Examine  it  carefully 
as  to  color  and  luster.  Explain,  giving  an  equation  to  express  the 
chemical  change. 

Finally  test  the  residue  by  adding  2  or  3CC  HN03,  noting  the 
color  of  the  fumes  and  of  the  residue.  See  whether  HN08  has  a 
similar  effect  on  the  original  mixture  of  CuO  and  C.  What  does 
the  test  show  ? 

II.  Carbon  a  Decolorizer. 

Shake  up  5  or  10g  of  bone  black  —  animal  charcoal  —  in  a  t.t, 
or  rec.  with  10  or  20CC  cochineal  sol.,  then  filter  and  notice  the  color 
of  the  liquid.  If  not  perfectly  colorless  pour  it  again  on  the  same 
filter,  using  more  carbon  if  needed.  Try  in  the  same  way  sols,  of 
indigo  and  litmus  ;  also  of  K2Cr207  and  K  Mn04.  Can  you  draw 
any  general  inference  of  the  decolorizing  action  on  animal,  vege- 
table, and  mineral  pigments,  the  first  three  being  animal  or  vege- 
table, the  last  two  mineral  ?  K2Cr207  may  be  turned  slightly  yellow 
by  alkali  in  the  bone  black. 

III.  Carbon  a  Deodorizer  or  Disinfectant. 

Prepare  a  sol.  of  H2S  (Exp.  42).  Notice  the  odor  of  the  gas  and 
its  solubility.  Put  into  a  rec.  5  or  10g  of  powdered  charcoal  and 
pour  upon  it  10  or  20CC  H2S  sol.  and  shake  the  mixture  well.  Then 
pour  the  whole  on  a  filter,  collect  the  filtrate  in  a  clean  t.t.  and  see 
if  any  odor  remains  ;  if  so,  mix  and  filter  again,  using  more  char- 
coal if  necessary.  The  H2S  has  been  absorbed  physically  into  the 
pores  of  the  coal  and  partially  oxidized  there.  This  illustrates  the 
absorbent  action  of  charcoal  on  gases,  animal  effluvia,  and  micro- 
organisms in  the  sick  room. 


17.     EXPERIMENTS  IN  COMBUSTION. 

I.  Structure  of  Flame. 

(1)  Make  a  careful  examination  of  the  parts  and  colors  of  a 
candle  flame,  and  make  a  drawing  to  show  them.  Move  the  candle 
slightly  in  the  air  to  show  the  outer  flame.  This  is  best  seen  in  a 
dark  room.  Describe  fully.  (2)  Examine  the  structure  of  a 
Bunsen  burner  (unscrew  the  top  if  necessary),  make  a  drawing  to 
show  the  orifices,  and  state  what  use  they  subserve.  Keplace  the 
tube  and  light  the  gas.  Hold  the  flame  in  front  of  a  dark  object 
(as  a  blackboard),  examine  the  parts,  make  a  drawing,  give  a  brief 
description,  and  state  the  color  of  each  part.  If  possible,  put  the 
flame  in  direct  sunlight,  and  study  the  parts  from  its  shadow,  to 
confirm  your  results. 

II.  Combustion  of  Flame, 

(1)  Put  a  moist  stick  across  the  base  of  the  Bunsen  flame  for  an 
instant,  and  notice  what  parts  are  burned.  Hold  a  stick  just  above 
the  inner  cone  of  the  flame.  Make  sketches  of  results.  (2)  Press 
quickly  down  on  the  flame  with  a  paper,  or  pasteboard,  remove 
before  it  burns,  and  notice  the  shape  of  the  charred  part,  or  press 
down  on  the  flame  with  a  fine  wire  gauze,  and  observe  by  the 
glowing  of  the  wire  where  the  heat  is  most  intense.  Sketch. 

(3)  Put  one  end  of  a  small  d.t.  into  the  inner  blue  cone,  not  into 
the  lamp,  and  try  to  light  the  gas  at  the  other  end.  (4)  Thrust  a 
match  quickly  into  the  inner  cone  near  the  bottom.  If  done  quickly 
the  phosphorus  will  not  take  fire.  The  match  contains  a  supporter 
and  a  combustible.  Why  does  it  not  burn  ?  In  what  parts  of  the 
flame  does  combustion  occur  ? 

Supplementary.  —  Examine  :  (a)  an  ordinary  gas  flame  ;  (b)  the  flame  of  a 
kerosene  lamp  ;  (c)  the  flame  of  a  burning  splinter,  or  match,  holding  it  vertical 
and  breaking  off  the  charred  part  as  fast  as  it  forms.  Have  all  flames  practi- 
cally the  same  structure  ? 


18.    EXPERIMENTS  IN  COMBUSTION. 

III.  Light  of  Flame. 

(1)  Sprinkle  a  very  little  charcoal  dust  into  a  Bunsen  flame, 
and  note  any  change  of  light  or  color,  or,  better,  dip  a  fine  splinter 
into  powdered  charcoal  and  thrust  it  into  the  openings  at  the  base. 
Notice  flame.  (2)  File  a  nail  or  other  metallic  substance  over  the 
flame,  or  sprinkle  in  CuO,  or  "  iron  by  hydrogen."  (3)  Also  stir 
up  the  dust  near  the  flame,  or  tap  the  lamp  with  the  fingers.  What 
produces  flame  ?  What  is  the  cause  of  light  in  a  flame,  and  what 
flames  give  light  ?  (4)  Close  the  orifices  at  the  base  of  the  burner, 
and  explain  the  change  of  light.  (5)  Set  fire  to  a  small  piece  of 
charcoal,  by  holding  it  in  a  flame,  and  see  whether  it  burns  with 
flame  or  only  glows.  What  does  this  show  ? 

IV.  Kindling  Point. 

(1)  Light  the  gas  and  hold  a  fine  wire  gauze  3  or  4cm  above  the 
burner.  Why  does  it  not  burn  above  the  wire  ?  (2)  Extinguish, 
then  relight  the  gas  above  the  gauze.  Result  and  explanation. 
Gradually  lift  the  wire  till  the  gas  will  not  burn.  (3)  Again  light 
the  gas  above  the  gauze,  and  hold  another  gauze  above  the  flame,  so 
as  to  confine  it  above  and  below.  State  three  conditions  of  combus- 
tion, define  each,  and  show  how  this  exp.  illustrates  them. 

Supplementary.  —  Why  does  a  lamp  smoke  ?  Why  does  phosphorus  take 
fire  spontaneously  ?  Why  does  gunpowder  explode  ?  Why  will  it  burn  with- 
out air  ?  Why  do  we  exclude  the  air  to  put  out  a  fire  ?  Why  does  blowing  a 
flame  sometimes  cause  it  to  burn,  and  sometimes  extinguish  it  ?  Why  does 
cannel  coal  burn  with  flame  ?  When  will  a  mixture  of  H  and  air  not  explode  ? 
Why  will  some  substances  burn  in  water  ?  See  which  has  the  lower  kindling 
point,  P  or  S,  by  putting  each  on  one  end  of  a  piece  of  iron  at  equal  distances 
from  a  flame  which  heats  the  other  end. 

Terms :  Kindling  temperature,  spontaneous  combustion,  combustible,  sup- 
porter. 


19.    POSITIVE  AND  NEGATIVE  ELEMENTS. 

I.  Dis,  Ag  in  HN03  and  ppt.  Ag  with  Cu. 

Put  a  ten-cent  silver  coin  into  an  e.d.  and  add  10  or  20  drops  of 
HN03.  Warm  it,  if  necessary,  over  asbestos,  and 
watch  the  result  as  to  action,  color  of  liquid,  color  of 
fumes,  etc.,  and  give  the  reason  for  each,  with  equa- 
tion. When  action  stops,  or  the  coin  is  dissolved,  add 
10CC  H20,  then  pour  it  into  a  t.t.  and  put  in  a  copper 
wire  (Fig.  23).  Leave  for  10  to  30  minutes.  At 
this  point  begin  II.,  but  observe  any  deposit  on  the 
wire,  noting  its  color,  luster,  texture,  crystalline 
form,  and  any  change  in  the  color  of  the  liquid.  Ex- 
plain, giving  equation.  Save  the  Ag.  Which  has 
greater  affinity  for  N  03,  H,  or  Ag  ?  Why  is  H  not  set  free  ? 

II.  Dis.  Cu  in  HN03  and  ppt.  Cn  with  Pb. 

Put  into  a  t.t.  or  e.d.  a  thin  piece  of  sheet  Cu,  say  l<icm;  add  10  or 
20  drops  HN03.  Make  as  accurate  observations  and  notes  as  be- 
fore, including  equation.  After  dissolving  the  Cu  add  10CC  HaO, 
and  put  in  a  Pb  wire  (or  other  piece  of  Pb),  made  bright  with  a 
file  or  by  just  dipping  it  into  a  little  HN03.  Leave  it  for  some 
time  in  the  Cu  (NO3)2  sol.,  and  begin  III.  Afterwards  notice  the 
deposit,  the  color  of  liquid,  etc.,  as  before,  and  take  full  notes  with 
equations.  Which  has  more  affinity  for  N  03,  Cu,  or  Ag  ? 

III.  Dis.  Pb  in  HN03  and  ppt.  Pb.  with  Zn. 

Dis.  part  of  a  small  piece  of  Pb  in  a  few  drops  of  H  N  03,  heat- 
ing if  necessary,  and  when  Action  ceases  add  10CC  H20  ;  pour  the 
liquid  into  a  t.t.  and  put  in  a  piece  of  Zn.  There  should  be  scarcely 
any  free  acid  when  the  Zn  is  introduced,  or  violent  effervescent 
action  will  ensue  and  both  Pb  and  Zn  will  dissolve.  Make  full 
notes  as  before,  including  equations. 

Supplementary.  —  (a)  Obtain  crystals  of  pure  AgN03  from  a  coin,  (b)  Of 
Pb(NO3)2  from  Pb.  (c)  Of  Cu(NO3)2  from  Cu.  (d)  Make  CuSO4  from  Cu  with 
dil.  acid,  (e)  See  whether  Zn  will  ppt.  Cu  from  CuSO4.  (f)  From  CuCl2. 
With  loz  of  pure  Ag,  how  much  AgNO3  could  be  made  ?  How  much  Ag  will 
5s  of  Cu  replace  from  a  sol.  of  AgN  O3  ? 

Terms:  Chemical  solution,  physical  solution,  precipitation,  stochiornetry. 


2O.  ACIDS,  BASES,  SALTS. 

I.  Acids, 

(1)  Pour  into  an  e.d.  a  few  drops  of  HC1,  add  4  or  5CC  H20,  stir 

it,  taste  a  drop  from  the  s.r. 
(Fig.  24).  Dip  the  end  of  a 
strip  of  blue  litmus  paper  into 
it.  State  results.  (2)  Einse 
the  e.d.,  then  put  in  a  few- 
drops  HN08  and  5CC  H20,  stir 
24.  and  test  as  before,  (3)  Test 

in  like  manner  H2S  04.     What  do  these  exps.  teach  you  of  acids  ? 

II.  Bases. 

(1)  Pour  into  an  e.d.  1  or  2CC  NH4OH,  add  4  or  5CC  H20,  stir  it, 
and  taste  a  drop.  If  it  has  no  taste  add  more  NH4OH.  Dip  the 
end  of  a  piece  of  red  litmus  paper  into  it.  (To  redden  blue  litmus 
hold  it  in  the  fumes  of  H  Cl.  To  turn  red  litmus  paper  blue  hold 
it  in  NH3  fumes.)  (2)  Einse  the  e.d.  and  test  NaOH  sol.  in  the 
same  way.  Also  (3)  KOH  sol.  What  do  these  exps.  teach  con- 
cerning bases  ? 

III.  Salts. 

(1)  Pour  into  a  clean  e.d.  1  or  2CC  of  Nad  sol.,  taste  a  drop  of 
it,  and  test  it  with  litmus,  red  and  blue.  Test  in  the  same  way 
(2)  KN08  sol.,  also  (3)  a  sol.  of  (N  H4)2S  04.  What  is  the  usual 
action  of  salts  on  litmus  ?  Test,  however,  these  sols,  with  both 
colors:  (4)  Na2C03;  (5)CuS04;  (6)  HNaC03;  (7)  HNaS04. 

Supplementary.  —Test  sols,  of:  (a)  H3PO4  ;  (b)  H2C204  ;  (c)HC2H3O2r 
(d)  Ca  (OH)2  ;  (e)  Ba  (OH)2  ;  (f)  HNa2PO4  ;  (g)  Na2B407  ;  (h) 


Terms  :  Acid,  base,  salt,  acid  salt,  normal  salt,  alkaline  salt,  neutral  salt, 
salt  acid  to  litmus,  alkali,  fixed  alkali,  volatile  alkali,  alkaline  carbonate. 


21.    ACID,  ALKALINE,  AND  NEUTRAL  REACTIONS. 

Put  into  a  small  beaker  or  a  t.t.  5CC  of  an  aqueous  sol.  of  blue 
litmus.  (1)  Pour  a  few  drops  of  HC1  into  an  e.d.,  beaker,  or  t.t. 
and  dip  a  s.r.  into  this  (never  dip  a  rod  into  a  reagent  bottle),  then 
stir  the  litmus  solution  with  it,  noting  any  change  of  color.  If 
none  occurs  add  another  drop  of  acid  with  the  rod.  (2)  Pour  a 
few  drops  of  NH4OH  into  a  clean  e.d.  or  t.t.,  dip  the  s.r.  into  it, 
then  stir  the  litmus  solution  with  this.  If  the  color  is  unchanged 
repeat  till  blue  is  again  obtained.  (3)  In  the  same  way  put  a  drop 
(or  more,  if  necessary)  of  HN03  from  an  e.d.  into  the  same  blue 
solution.  (4)  When  it  is  reddened  add  a  drop  or  more  of  NaO  H 
sol.  until  it  becomes  blue.  (5)  Change  it  again  to  red  with  a  drop 
of  H2S04>  and  (6)  restore  the  color  with  KOH  sol. 

Supplementary.  —  (a)  Add  a  few  drops  of  H2O  to  a  sol.  of  red  litmus,  and 
also  to  one  of  blue,  (b)  Add  to  both  red  and  blue  litmus  sols,  a  sol.  of  NaCl. 
(c)  Try  N  H4C1  sol.  (d)  K  N  08  sol.  (e)  H  NaC  O3  sol.  (f )  H  K  S  O4.  (g)  CuS  O4. 

Terms :   Acid,  alkaline,  and  neutral  reactions. 


22.  SOLUBLE  SALTS  BY  NEUTRALIZATION. 

I.  Sodium  Chlorid. 

Pour  into  an  e.d.  not  over  5CC  NaOH  sol.,  and  into  a  clean  t.t.  or 

beaker  4  or  5CC  HC1.  Now  add 
some  of  this  latter,  a  little  at  a 
time  (Fig.  25),  to  the  NaOH 
sol.,  stirring  it  meantime  till 
the  product  is  neutral  to  litmus 
paper  ;  when  nearly  neutral 
add  a  drop  at  a  time  with  a 

s.r.  and  test  with  both  colors,  using  only  the  end  of  the  paper  and 
keeping  it  on  the  side  of  the  e.d.  If  blue  litmus 
paper  is  reddened  by  the  sol.,  add  NaOH  sol.,  a  few 
drops  at  a  time.  If  red  litmus  is  turned  blue  add  a 
drop  of  H  Cl.  When  the  sol.  does  not  affect  either 
red  or  blue  litmus  left  in  it  for  a  minute,  show  it 
with  both  papers  in  it  to  the  instructor,  then  filter 
and  evaporate  the  liquid  to  dryness  by  boiling  it  over 
a  plate  and  abestos  paper  (Fig.  26).  When  it  is  cool, 
examine  the  residue  and  taste  it.  What  is  the  object 
of  evaporation  ?  Explain  what  took  place  when  the  acid  and  base 
were  mixed,  and  give  the  equation  to  express  it.  Sift  a  little  of 
the  salt  into  the  flame.  The  color  shows  a  cpd.  of  Na.  Test  for 
Cl  by  Exp.  27. 

II.  Potassium  Sulfate. 

Into  an  e.d.  put  5CC  KOH  sol.  and  neutralize  it  with  dilute 
H2S04,  using  both  test  papers.  When  sure  it  is  neutral,  evaporate 
most  of  the  water  and  taste  the  product.  Explain  the  action,  giving 
the  equation.  Sift  a  little  into  a  flame.  The  color  shows  a  K  cpd. 
(best  seen  through  blue  glass).  Test  S04  by  Exp.  31. 

III.  Ammonium  Nitrate. 

Neutralize  NH4OH  with  HN03  (preferably  dilute)  in  the  same 
way  as  before.  Stop  evaporation  when  dense  fumes  begin  to  ap- 
pear. These  fumes  indicate  a  decomposition  of  the  salt  by  heat 
(v.  Exp.  34). 


Supplementary.  —  How  would  you  make  by  neutralization  NaN  Os, 
K  N  O3,  K  Cl,  N  H4C1,  (N  H4)2S  O4  ?  Write  also  equation  for  each.  Weak  acids 
will  not  neutralize  strong  bases,  and  vice  versa.  Hence,  salts  like  NaaC  O8  are 
not  neutral.  How  do  these  exps.  illustrate  the  law  of  definite  proportion  ? 

Terms  :  Neutralization,  double  decomposition,  definite  proportion,  evapora- 
tion, fumes. 


23.    SOLUBLE  SALTS  FROM  METALS. 

I.  Zinc  Chlorid. 

To  a  piece  of  Zn  in  a  t.t.  add  water  and  a  little  HC1.  Describe 
and  explain  the  action,  and  when  it  ceases,  pour  the  liquid  into  an 
e.d.  and  evaporate  to  dryness.  Observe  and  taste  the  salt.  Name 
it  and  write  the  equation.  To  test  the  salt,  add  a  little  H2O  to  dis- 
solve it  and  divide  the  sol.  into  4  parts.  Test  for  Cl  by  Exp.  27, 
and  for  Zn  by  Exp.  70. 

II.  Iron  Sulfate. 

Dissolve  as  above  a  few  Fe  filings  in  dil.  H2S  04.  When  action 
stops  add  H2O,  filter,  and  evaporate  the  filtrate.  Then  dissolve  the 
salt  in  water  after  having  examined  it.  Name  it  and  write  the 
equation.  Test  it  for  Fe  by  Exp.  63,  and  for  S  04  by  Exp.  31. 

III.  Copper  Nitrate. 

Dissolve  a  little  Cu  in  dil.  H  N  03,  pour  off  the  liquid,  evaporate, 
and  then  add  H20.  Test  for  Cu  by  Exp.  56.  and  for  N03  by  82. 
Make  full  notes. 

Supplementary.  —  The  salts  in  Exps.  22,  23  are  sol.  in  water.  Insoluble 
salts  are  not  made  in  this  way.  PbCl2  is  only  partially  insoluble,  hence  HC1 
will  not  dissolve  much  Pb.  Table  A  shows  that  there  are  but  two  soluble  salts 
of  Pb ;  hence  most  acids  do  not  act  upon  that  metal.  By  reference  to  this 
table  you  can  judge  what  acids  will  probably  act  on  a  given  metal.  Will  H2S  O4 
dis.  Ba?  Pb?  Cu?  Will  H  Cl  probably  dis.  Sn  ?  Ag?  Hg?  Mg?  Will  H3P04 
dis.  Pb?  Ca?  Ag?  (a)  Try  any  of  the  above.  (b)  Try  .to  dis.  Pb  in 
HC2H8O2.  Compare  chemical  sol.,  as  shown  in  23,  with  physical  sol.,  Exp.  4. 
What  two  processes  in  chemical  sol.? 

Terms :  Insoluble,  soluble,  saturation,  supersaturation. 


24.     SOLUBLE    SALTS    FROM    CARBONATES, 
HYDROXIDS,  OXLDS. 

I,  Carbonates. 

(1)  To  a  piece  of  CaC03  (marble  or  limestone)  in  a  t.t.  add 
H20,  and  a  little  H  Cl.  When  the  action  stops,  pour  a  little  of  the 
liquid  into  an  e.d.,  evaporate  and  notice  the  residue.  See  if  it  will 
dis.  in  H20.  State  your  observations  and  the  reaction.  Test  for 
the  presence  of  Ca  by  Exp.  74.  (2)  Try  Na2C03  (or  HNaC03) 
with  HC1.  (3)  CaC03  may  be  tried  with  H2S04  or  HN03. 

II.  Hydroxids. 

(1)  To  some  Fe(OH)3  (made  by  adding  NH4OH  to  FeCl3  sol., 
and  pouring  off  the  supernatant  liquid  after  the  ppt.  settles)  add 
drop  by  drop  just  enough  HC1  to  dissolve  it.  (2)  Try  also  HNO3 
and  H2S04  on  separate  ppts.  of  Fe(OH)3.  Evaporate  and  dis.  in 
H20  as  before.  Test  for  Fe  by  Exp.  63.  (3)  Try  A1(OH)3  (made 
from  A1C13  sol.  and  NH4OH)  with  HC1.  Evaporate,  dis.  in  H2O, 
and  test  for  Al  by  Exp.  64. 

HE.  Oxids. 

To  28  PbO  (litharge)  in  an  e.d.  add  some  dil.  HN03  and  heat 
it.  Decant  on  a  filter,  partly  evap.  the  filtrate,  add  H20,  and  test 
for  Pb  by  Exp.  48. 

Supplementary.  —  Notice  from  Table  A  what  carbonates  and  hydroxids  are 
soluble,  (a)  Add  H20  to  a  little  Na2CO3  (or  K2C03)  in  a  t.t.  and  boil  a 
minute,  (b)  In  another  tube  cautiously  add  HC1  to  Na^COs..  Explain  the 
difference  between  (a)  and  (b).  (c)  Into  (a)  pour  cautiously  a  little  H  Cl.  De- 
scribe the  action  and  explain  it  with  reaction.  Sol.  salts  may  be  made  from 
many  other  classes  of  cpds.  besides  the  above. 

Terms :  Physical  and  chemical  solution,  decantation. 


25.    INSOLUBLE  SALTS  BY  PRECIPITATION. 

Insol.  Salts  of  Pb. 

(1)  Pour  into  a  t.t.  5CC  Pb(N03)2  sol.  and  add  a  few  drops  HC1. 
(2)  Try  it  again,  substituting  Nad  sol.  for  HC1.  (3)  Use  also  a 
sol.  of  N  H4C1.  Record  results  and  write  equations.  (4)  Now  in 
place  of  Pb(NO3)2  use  a  sol.  of  Pb(C2H302)2,  try  the  action  of  the 
same  three  reagents  as  previously  used,  and  make  a  similar  record. 
What  is  the  ppt.  in  each  case  ?  Could  you  obtain  the  same  ppt.  by 
putting  together  any  other  sols.,  and  if  so,  what  ones  ? 

To  5CC  of  each  of  the  following  sols,  in  a  t.t.  add  a  little  sol.  of 
Pb(N  03)2  or  Pb(C2H302)2  and  write  the  equation,  underlining  the 
ppt.  and  writing  the  color  above.  (5)  K2O04.  (6)  K  I.  (7)  K  Br. 
(8)  NaOH.  (9)  Na2C03.  (10)  Na2S04.  (11)  K4FeCy6. 

Supplementary.  —  What  are  the  only  two  soluble  salts  of  Pb  ?  Law  of 
Ppn. :  Whenever  a  mixture  is  made  of  two  sols.,  one  of  which  contains  the  positive 
part  and  the  other  the  negative  part  of  an  insoluble  cpd.,  a  ppt.  of  the  insol.  cpd. 
will  always  form. 

From  Table  A  what  salts  of  Ba  are  insol.  ?  (a)  Try  to  make  some  of  them 
by  the  application  of  the  above  law.  (b)  Also  try  Fe(0  H)3.  (c)  Make  HgS. 
(d)  Try  to  make  MnS.  (e)  Make  CaC  O8. 

Terms:  Insoluble,  precipitation,  positive,  negative. 


26.    HYDROCHLORIC  ACII>,  HC1. 

Preparation. 

(1)  Fill  2  recs.  %  full  of  water.  Connect  the  apparatus  as  in  Fig. 
27,  observing  how  the  tubes  extend.  (A 
safety-tube  may  also  be  used  if  desired.) 
Then  put  into  a  flask  10g  NaCl  (preferably 
fused)  and  20CC  H2S04  which  has  previ- 
ously been  mixed  with  5CC  of  H20.  Be 
sure  you  have  enough  acid,  or  the  flask  is 
liable  to  crack.  Heat  slowly  for  10  or  15 
minutes  over  asbestos,  but  do  not  let  the 
froth  extend  to  the  neck  of  the  flask.  Look 
for  any  current  in  the  liquid  of  the  rec. 
and  explain.  (2)  Detach  the  apparatus 
(at  a,  Fig.  27)  and  pass  some  of  the  escap- 
ing gas  over  a  few  drops  of  NH4OH  in  an  e.d.  (If  much  gas  is 
accidentally  breathed,  inhale  NH3.)  Describe  the  fumes  (note 
whether  they  have  any  odor  different  from  H  Cl  or  N  H3),  name 
them,  state  the  color,  and  write  the  equation  for  their  production. 
This  is  the  ammonia  test  for  H  Cl.  Ascertain  whether  the  product 
is  gaseous,  or  solid,  by  dipping  a  rod  into  strong  H  Cl  and  holding  it 
over  a  bottle  of  NH4OH.  (3)  Pass  some  of  the  gas  from  the  gen. 
into  a  sol.  of  blue  litmus.  What  does  this  show  as  to  the  solubility 
of  HC1  ?  What  else  does  it  show  ? 

Supplementary.  —  How  would  you  test  for  the  presence  of  N  H8  ?  Generate 
HC1  if  possible  from  :  (a)  KC1 ;  (b)  NH4C1,  using  an  open  t.t.  and  applying  the 
usual  tests,  (c)  Try  PbCl2.  Law  of  Formation  of  Gases  :  When  two  substances, 
which  can  react  so  as  to  liberate  a  gas,  are  put  together,  that  reaction  will  always 
take  place  and  the  gas  be  formed. 


Fig.  27. 


Terms :  Wolff  bottle,  flask,  safety -tube,  muriatic  acid. 


27.    HYDROCHLORIC  ACID,  HC1. 

Properties  and  Tests, 

(1)  Test  the  liquid  in  each  bottle  (Exp.  26)  with  blue  litmus 
paper.  (2)  Taste  a  drop,  using  a  s.r.  (3)  Cautiously  note  the  odor. 
(4)  Put  a  piece  of  Zn  into  a  t.t.  and  pour  over  it  5  or  10CC  of  the 
contents  of  the  first  Wolff  bottle.  (5)  If  a  gas  escapes,  test  its 
combustibility.  Explain  fully  with  observations  and  equations. 
(6)  Put  into  a  t.t.  5CC  Pb(N  08)2  sol.  and  add  a  little  of  the  liquid 
from  the  first  bottle.  If  a  ppt.  falls,  pour  a  small  part  of  it  into 
another  t.t.,  add  a  little  H20,  and  boil  a  minute.  Does  it  dissolve  ? 
What  does  that  show  ?  Now  add  a  little  K2Cr207  (or  K2Cr04)  sol. 
Explain.  (7)  To  5CC  AgN  03  sol.  add  a  little  of  the  acid.  If  a  ppt. 
falls  let  it  settle,  then  pour  off  most  of  the  supernatant  liquid, 
leaving  the  residue  ;  then  add  N  H40  H  and  shake  it.  Finally 
acidify  cautiously  with  HN03.  Explain  all  results.  (8)  Test 
HgN  03  sol.  in  the  same  way,  adding  N  H40  H  at  the  end,  but  not 
HN03.  By  any  of  the  above  exps.  can  you  determine  which  bottle 
contains  the  stronger  acid  ? 

Supplementary. — (a)  Add  HC1  to  Cu(NO3)2  sol.  and  explain  the  result, 
(b)  Separate  Ag  from  Cu  in  a  mixture  of  solutions  of  their  nitrates.  Try  the 
action  of  HC1  on  sols,  of  :  (c)  Co(NO3)2  ;  (d)  NaNO3  ;  (e)  KN03  ;  (f)  MgSO4. 
What  3  chlorids  are  insol.  in  H2O,  and  how  are  they  made  ? 

Terms :  Analysis,  reagent,  pungent,  acidify,  alkalize. 


28.    ETCHING  WITH  HYDROFLUORIC  ACID,  HF. 

Cover  thinly  with  beeswax  or  paraffin  one  side  of  a  small  piece 
of  glass.  Spread  the  wax  evenly  over  the  surface, 
by  warming  the  other  side  of  the  glass  and  pour- 
ing off  the  excess  of  melted  wax.  With  a  sharp 
metallic  point,  as  the  handle  of  a  file,  mark 
Fig.  28.  some  design  through  the  wax  when  cold  (Fig. 

28).  Put  into  a  lead  dish  (it  will  spoil  a  porce- 
lain e.d.)  a  very  little  HF  sol.  (be  exceedingly  careful  not  to  get 
any  on  the  flesh)  and  with  a  camel's-hair  brush  spread  some  of  it 
over  the  design  on  the  glass.  Do  this  several  times.  Finally, 
after  a  few  minutes  wash  away  the  acid  from  the  glass,  melt  and 
pour  off  the  wax,  wiping  off  what  remains  with  a  cloth  wet  in 
naphtha,  or  alcohol.  Examine  closely  the  result  and  describe  it. 
By  reason  of  its  affinity  for  Si02,  HF  acts  on  the  glass  and  forms 
SiF4.  The  equation  should  be  written. 

Supplementary.  —  Etch  a  t.t.  so  as  to  make  a  graduate  of  it.  Why  cannot 
H  F  sol.  be  kept  in  glass  bottles  ?  H  F  is  made  by  treating  powdered  CaF2 
(fluorite)  with  H2S  04  in  a  lead  dish.  Write  the  equation  (v.  Exp.  89  for  other 
tests).  The  fumes  must  not  be  inhaled. 

Terms :   Etching,  fluor  spar,  fluorid,  fluorite,  silica. 


29.    NITRIC  ACID,  HNO8. 


Fig.  29. 


I.  Preparation. 

Introduce  into  a  glass    retort   through   the    tubulure,   holding 

the  foi*mer  so  as  not  to  have  the 
chemicals  touch  the  neck  of  the 
retort  (Fig.  29),  10  or  15*  fine 
NaN08  (or  KN03)  and  20  or  25CC 
3H2S04. 

Adjust  the  apparatus  as  in 
Fig.  30,  having  the  neck  of  the 
retort  pass  to  the  bottom  of  a  wide 
t.t.,  which  is  surrounded  by  water 
in  a  wide  tumbler,  or  bottle.  The 
water  is  to  cool  and  condense  the 
acid  from  the  vaporous  state  in 
which  it  passes  over.  Apply  the 
Bunsen  flame,  using  a  plate  and  as- 
bestos, for  15  or  20  minutes.  Notice 
the  liquid  running  down  the  neck  of 
the  retort,  also  any  colored  fumes  — 
name  and  account  for  the  latter,  and 
see  whether  they  increase  with  the 
heat  —  the  color  of  the  liquid  in  the 
t.t.,  and  the  cause  of  it.  Do  the  ordi- 
nary reactions  (which  should  be  writ- 
ten) account  for  the  fumes  ?  Observe 
also  the  color  of  the  product  in  the 
retort.  Heat  may  have  reduced  some 
of  the  white  Na2S04  to  dark-colored 
Na2S.  Use  great  care  not  to  get  any 
of  the  acid  on  the  hands.  The  anti- 
dote, after  thorough  washing,  is  HNaC03  (v.  Eule  19). 

II.  Tests. 

(1)  Test  the  vapor  from  the  end  of  the  retort  with  a  few  drops 
of  N  H40  H.  (2)  Put  a  drop  or  more  of  the  acid  on  a  very  few  Cu 
filings  in  an  e.d.  Observe  and  explain  with  equation.  (3)  Try 
with  a  s.r.  the  action  of  a  drop  on  the  finger-nail,  then  wash  it  off 
and  add  a  drop  of  NH4OH.  This  shows  its  action  on  animal  mat- 
ter. (4)  Try  it  also  on  a  feather  or  on  silk.  (5)  Try  its  decolor- 
izing action  on  3  or  4CC  of  indigo  sol.  in  a  t.t.  Try  its  action  on 
insoluble  salts,  e.g.:  (6)  CuS  ;  (7)  CaC08 ;  (8)  BiOCl.  State  what 
this  shows  of  the  solubility  of  the  respective  nitrates  (v.  alsoExp.  82). 

Supplementary.  —  (a)  Compare  the  action  of  H  N  O3  and  H2S  O4  on  wood. 
Could  HNO3  be  made  from  Pb(NO3)2?  How  are  nitrates  made?  (b)  Make 
Zn(NO8)2.  (c)  Try  to  dis.  a  little  Sn  in  HN  03  in  an  e.d.  (d)  Try  Sb.  (e)  Put 
a  drop  of  commercial  HNO3  on  writing  paper,  another  on  newspaper.  The 
latter  contains  wood  pulp,  (f)  Try  to  decolorize  anilin  solutions. 

Terms:  Fuming  nitric  acid,  metastannic  acid,  xanthoproteic  acid,  salt  of 
nitric  acid,  nitrate,  tubulure. 


Fig.  30. 


30.    AQUA  REGIA. 

I.  Preparation. 

Pour  2  or  3CC  of  HISTOg  into  a  t.t.  containing  6  or  8CC  of  HC1. 
If  there  is  no  evidence  of  chemical  action,  warm  the  mixture  a 
minute  and  observe.  To  what  is  the  color  due  ?  Give  reaction. 

II.  Tests. 

(1)  Into  a  part  of  the  aqua  regia  introduce  a  little  gold  leaf  by 
winding  it  around  a  moist  s.r.,  not  letting  it  touch  the  sides  of  the 
t.t.  (2)  Into  another  part  drop  a  bit  of  Pt  foil,  £qcm.  If  no  action 
ensues,  heat  it.  Pt  does  not  dis.  as  readily  as  Au.  Try  the 
solvent  action  of  aqua  regia  on  :  (3)  Zn  ;  (4)  Fe  ;  (5)  Cu  ;  (6)  Pb. 
Give  the  usual  explanations,  reactions,  etc.,  for  each  of  the  above 
exps.  Why  should  not  the 'acid  act  as  well  on  Pb  as  on  the  others  ? 

Supplementary.  —  See  if  Au  will  dis.  in  :  (a)  HC1,  or  (b)  HNO3.  Also  try 
(c)  Pt.  Try  Hg  in  (d)  H  Cl,  then  in  (e)  aqua  regia.  (f )  Try  Fe  in  each  and 
notice  the  color  of  each  liquid  after  filtering.  Explain,  (g)  Test  the  2  chlorids 
of  Fe  by  Exp.  63. 

Terms :  Nitro-hydrochloric  acid,  gold  chlorid,  ferrous  and  ferric  chlorids. 


31.    SULFURIC  ACID, 


I,  Preparation. 

Burn  a  small  piece  of  S  in  a  rec.  in  which  there  is  H20  enough 
to  cover  the  bottom,  using  a  d.s.  and  confining  the  fumes  as  much 
as  possible  by  covering  the  mouth  of  the  rec. 

Pour  into  an  e.d.  1  or  2CC  HN03,  and  dip  into  this  a  piece  of 
strong  paper,  or  cloth,  or  a  wood  shaving,  and  lower  it  into  the  rec. 
of  S  02,  holding  it  there  for  some  time  without  dropping  any  acid 
from  it  into  the  rec.  See  whether  the  fumes  change  color.  Repeat 
the  operation  several  times.  Explain  the  phenomena  and  give  all 
reactions.  Cover  the  rec.  with  the  hand  and  shake  the  liquid  and 
the  gases  well  together. 

II.  Tests. 

(1)  Apply  the  litmus  test.  (2)  Put  a  drop  of  the  liquid  on 
writing  paper,  and  evaporate  it  so  as  not  to  burn  the  paper.  See 
whether  the  paper  is  charred,  blackened,  or  made  rotten  by  the 
liquid.  Explain.  This  is  a  test  for  free  H2S04.  (3)  Add  a 
little  of  the  liquid  to  5  or  10CC  BaCl2  sol.  (or  Ba(N03)2)  in  a  t.t., 
state  the  effect  and  give  an  equation.  If  you  obtain  a  ppt.,  add  a 
little  H  Cl  and  shake  it  well.  Does  it  dissolve  ?  (4)  Pour  into  a 
t.t.  containing  5CC  H2O  the  same  amount  of  H2S  04  from  the  shelf 
bottles.  Observe  any  thermal  effects  on  this  mixture  and  explain. 
Save  the  dilute  acid  in  a  separate  rec.  (5)  Apply  tests  (2)  and  (3) 
above  to  this  mixture.  (6)  Pour  a  few  drops  of  concentrated  acid 
upon  1  or  2g  sugar  in  an  e.d.  (7)  Dip  a  small  stick  into  a  t.t.  which 
contains  1  or  2CC  H2S  O4.  (8)  Pulverize  a  bit  of  starch,  add  a  few 
drops  of  the  acid.  If  no  change  occurs,  cautiously  heat  it  for  a 
minute.  Sugar  is  C12(H20)n  ;  starch  is  C6(H20)5  ;  cellulose  is 
C18(H20)15  ;  explain  the  action  of  the  acid. 

Supplementary.  —  Why  is  commercial  H2S  O4  liable  to  be  of  a  brown  color  ? 

(a)  Measure  accurately  10CC  of  concentrated  acid  in  a  graduate,  leave  it  in 
an  open  t.t.  or  rec.  for  a  week,  then  measure  it  carefully  again.  Explain  the 
result,  (b)  Test  commercial  acid  for  PbS04  by  pouring  a  little  into  an  equal 
vol.  of  H2O  in  a  t.t.  BaSO4  is  the  only  salt  of  Ba  that  is  not  dis.  by  HC1. 
(c)  Test  Na2SO4  sol.  with  BaCl2.  Explain,  (d)  Test  a  sol.  of  Na2SO3  for 


Terms  :   Salt  of  sulfuric  acid,  fuming  sulfuric  acid,  sulfate,  starch,  cellulose. 


32.    AMMONIUM  HYDBOXID,  NH4OH;  AMMONIA,  NH3. 


I.  Preparation, 

Powder  and  put  into  a  flask  about  10* 
NH4C1  and  7«  Ca(OH)2  (freshly  slaked  is 
best).  Add  20CC  H20  and  connect  with 
Wolff  bottles  containing  H20  (Fig.  31), 
as  in  the  HC1  exp.  Heat  10  or  15 
minutes,  using  a  plate  and  asbestos  paper. 
Observe  the  phenomena,  especially  the 
pressure  in  the  different  bottles  and  the 
absorption  of  gas,  and  write  the  reaction. 
While  the  mixture  is  heating,  do  III. 


Fig.  31. 


II,  Tests. 

(1)  Disconnect  the  flask  while  the  gas  is  escaping  (a,  Fig.  31) r 
put  2  or  3  drops  HC1  into  an  e.d.,  and  pass  the  gas  over  it  from  the 
gen.  Observe  the  fumes,  giving  equation.  (2)  Let  the  flask  cool 
as  it  stands,  and  test  the  liquid  in  each  bottle  (odor  and  litmus). 
Put  sols.  (5CC  each)  of  the  following  substances  into  separate  tubes, 
and  add  a  little  of  the  prepared  liquid  to  each  :  (3)  FeS  04 ; 
(4)  FeCl3  ;  (5)  A1C18.  Observe  colors,  especially  -of  ferrous  and 
ferric  cpds.  (6)  Test  likewise  CuCl2  sol.,  first  with  very  little 
NH4OH,  then  with  excess.  State  and  explain  all  phenomena. 

III.  Ammonia. 

Mix  2  or  3*  of  fine  NH4N03  with  an  equal  quantity  of  Ca(OH)2, 
put  them  into  a  t.t.,  and  warm  it  over  a  flame.  See  whether  a  gas 
escapes  by  :  (1)  cautiously  taking  the  odor  ;  (2)  testing  with  red 
litmus  paper  ;  (3)  with  H  Cl. 

Supplementary.  —  (a)  Put  into  a  t.t.  a  gram  or  two  of  either  (NH4)2SO4r 
N  H4NO3,  NH4C1,  or  (NH4)2C2O4,  and  add  a  little  NaOH  (or  KO  H)  sol.,  warm 
it,  and  apply  tests.  What  two  classes  of  cpds.  are  used  to  obtain  ammonia  ? 
Are  the  above  examples  of  double  decomposition,  and  why  ?  Relation  between 
ammonia  and  ammonium  hydroxid  ?  (b)  Fill  a  t.t.  with  NH8  by  upward  dis- 
placement, and  invert  it  over  a  rec.  of  water.  Observe  and  explain. 


Terms :  Volatile  alkali,  fixed  alkali. 


33.    FIXED  ALKALIES. 

I,  Sodium  Hydroxid,  NaOH. 

To  5CC  of  a  saturated  sol.  of  Na2C03  add  about  an  equal  quantity 
of  Ca(0  H)2  sol.  Shake  the  mixture  well  and  observe.  If  a  ppt. 
falls,  name  it  and  write  the  equation.  What  goes  into  solution  ? 
Let  the  ppt.  settle,  then  add  some  of  the  supernatant  liquid  to  sols. 
of  :  (a)  Fe(S04)  ;  (b)  FeCl3 ;  (c)  A1C13.  Effects,  colors,  and  equa- 
tions should  be  given  in  each  case.  If  any  effect  different  from 
what  is  expected  occurs,  it  should  be  noted  and  explained. 

II.  Potassium  Hydroxid,  KOH. 

Treat  a  sat.  sol.  of  K2C  08  in  precisely  the  same  way  as  Na2C  03 
above,  making  close  observations  and  taking  full  notes  as  before, 
including  all  the  tests  given. 

Supplementary.  —  Compare  the  action  of  fixed  alkalies  with  that  of  N  H4O  H 
on  sols,  of  Fe  and  Al  salts,  (a)  Obtain  some  NaO  H  or  KO  H  in  the  solid  state. 
In  what  other  ways  were  NaO  H  and  KOH  made  in  the  laboratory  ?  (b)  Would 
Ca(OH)2actonNaCltoformNaOH?  (c)  Ca(0  H)2  on  Na^S  O4  ?  (d)  Is  FeCl3 
sol.  acid,  alkaline,  or  neutral  ?  (e)  Is  A1(O  H)3  soluble  hi  excess  of  NaO  H  or 
KOH  sol.? 

Terms :  Hydroxid,  hydrate,  alkali  metals,  metals  of  alkaline  earths. 


Fig.  32. 


34.    OXIDS  OF  NITKOGEN. 

I.  Nitrogen  Monoxid,  N20  (Nitrous  Oxid). 

(1)  Put  into  a  flask  (of  200CC  capacity)  10*  of  NH4N  08,  not  too 

coarsely  crystalline  (so  as  not 
to  break  the  flask  in  melting). 
Connect  the  flask  with  a  large 
t.t.  (resting  in  a  rec.  of  H20, 
Fig.  32),  or  with  a  rec.  which 
contains  no  water  (Fig.  33),  and 
from  this  t.t.  or  rec.  have  a  d.t. 
leading  to  a  p.t,  so  as  to  collect 
the  gas  over  water.  Ha.ve  the 
joints  tight  and  the  tubes  pass 
through  the  stoppers.  Apply 
heat  not  too  rapidly,  notice  the 
order  of  changes  and  give  the 
main  reaction.  Are  there  any 
fumes  in  the  flask  ?  Is  the  gas 
colored,  and  why  ?  Obtain  2 
recs.  of  gas,  then  remove  the 
lamp  and  take  the  d.t.  from  the 
water,  letting  the  flask  cool  on 
the  r.s.  (2)  Taste  a  drop  of  the 
liquid  in  the  large  t.t.  or  rec., 
and  also  test  with  litmus,  red  and  blue.  Some  NH4N03  will 
probably  have  been  driven  over,  also  some  NO,  N02,  HN03,  etc., 
formed  by  breaking  up  of  NH4N03.  (3)  Test  the  gas  with  a  burn- 
ing stick,  also  with  a  glowing  one.  (4)  Test  the  combustibility  of  S 
(well  burning  when  introduced),  and  (5)  of  P.  Compare  the  bril- 
liancy of  flame  and  the  products  obtained  with  those  in  0,  and  write 
all  equations. 

Supplementary.  — Compare  the  action  of  heat  on  NH4N03  with  that  on 
Pb(N03)2  in  Exp.  10.  Compare  with  the  action  of  NaNO3  +  H2SO4  (Exp.  29). 
Learn  the  symbols  and  names  of  all  the  oxids  of  N.  Try  the  action  of  heat 
•  (using  a  t.t.)  on:  (a)  KN03  ;  (b)  Hg(N03)2;  (c)  Zn(NO3)2  ;  (d)  Pb(NO3)2. 


Fig.  33. 


Terms :   Laughing  gas,  nitrous  oxid,  nitrates,  nitrites. 


35.    OXIDS  OF  NITROGEN. 

II.  Nitrogen  Dioxid  NO  or  N202  (nitric  oxid). 

(1)  Arrange  the  app.,  with  inverted  recs.,  as  for  the  hydrogen 
exp.  Then  put  into  the  gen.  (or  t.t.)  5g  Cu  turnings,  cover  them 
with  water  and  add  through  the  thistle  tube  5CC  of  HN03.  Collect 
2  or  3  recs.  of  the  gas.  If  action  stops  add  a  little  HN03  (or  Cu,  if 
necessary).  Save  any  Cu  that  is  left.  Explain  the  different  colors 
of  the  gases  and  the  color  of  the  liquid.  (2)  Test  the  gas  with  a 
burning  stick.  Explain  the  fumes.  Test  also  with  (3)  S  and  (4)  P 
(well  burning).  In  (4)  see  whether  the  solid  gradually  separates 
from  the  gas.  Take  full  notes. 

III.  Nitrogen  Trioxid  N203  and  Tetroxid  N02  or  N204  (peroxid). 

(1)  Lift  a  rec.  of  the  gas  N  0,  just  prepared,  from  the  shelf  of 
the  p.t.  What  is  the  effect,  what  is  the  new  gas,  and  how  is  it 
formed  ?  (2)  Heat  1  or  2  crystals  of  Pb(N03)2  in  a  t.t.,  and  while 
the  gas  escapes  insert  a  glowing  stick  into  the  tube.  (3)  Put  a 
fragment  of  starch  into  a  t.t.  and  add  a  few  drops  of  HN03.  Heat 
cautiously. 

Supplementary.  —  State  how  the  oxids  of  N  are  derived  from  H  N  O3  and 
nitrates.  What  action  have  heat  and  reducing  agents  on  nitrates  ?  (a)  Notice 
the  action  of  direct  sunlight  on  strong  H  N  O3  in  stoppered  bottles,  (b)  Try  the 
action  of  heat  on  other  nitrates,  e.g.,  Cu(NO3)2,  KNO3.  (c)  Heat  a  bit  of 
powdered  charcoal  on  a  plate  or  asbestos,  and  when  it  is  hot  add  a  drop  of 
HN03  with  a  s.r.  N203  and  N02  are  both  red  and  not  distinguishable.  Find 
how  N2Og  is  prepared,  and  its  relation  to  HNO3. 

Terms :  Nitrous  and  nitric  anhydrids,  nitrogen  peroxid,  nitric  oxid. 


36.    CARBON  DIOXED,  CO2. 

I.  Preparation. 

Put  10  or  15g  CaC  03  (marble,  in  lumps)  into  a 
t.t.  or  gen.  (Fig.  34),  cover  with  H2O  and  —  after 
having  the  app.  all  prepared  —  add  5CC  HC1.  Add 
more  of  the  reagents  as  needed.  Enough  must  be 
used  to  produce  vigorous  action.  Attach  a  delivery 
tube  and  collect  a  rec.  of  gas  by  downward  displace- 
ment, having  the  tube  reach  to  the  bottom  of  the  rec. 
Fig.  34.  It  will  take  only  a  minute. 

II,  Tests. 

(1)  Test  the  gas  with  a  burning  stick.  (2)  Let  the  gas 
bubble  from  a  d.t.  into  5CC  Ca(OH)2  sol.  in  another  t.t.  and  look  for 
a  ppt.  Let  the  action  continue  until  the  liquid  clears.  (3)  When 
the  sol.  is  clear,  boil  it  for  a  minute  and  notice  the  reappear- 
ance of  the  ppt.  Explain  all  the  phenomena  very  fully,  giving 
equations  at  the  proper  places.  (4)  Pass  the  gas 
into  a  sol.  of  blue  litmus.  (5)  Observe  the  Ca  flame 
(bring  the  open  mouth  of  the  C02  gen.  close  to  a 
Bunsen  flame).  Small  particles  of  CaCl2  are  carried 
up  by  the  gas.  (6)  Also  dip  a  stick  into  the  sol., 
hold  it  in  the  flame  and  notice  the  color.  (7)  Take 
2  or  3CC  Ca(0  H)2  sol.  in  a  clean  t.t.  and  breathe  into 
it  through  a  glass  tube.  What  does  the  result  show  ? 
(8)  Put  a  little  lime  water  into  an  e.d.  and  look  for 
a  scum  after  a  few  minutes  ;  or  draw  the  air  through 
a  rec.  of  lime  water  (Fig.  35),  by  suction,  applying 
The  air  enters  at  a,  and  any  C  02  is  drawn  through 


Fig.  35. 


the  lips  at  b. 

the  lime  water.     Explain. 

Supplementary.  —  (a)  See  whether  you  can  obtain  C  02  from  Na2C  03.  Use 
an  open  t.t.  and  test  the  gas  with  a  drop  of  Ca(0  H)2  sol.  on  a  s.r.  (b)  Use  also 
HNaC03.  (c)  K2CO3.  (d)  Test  some  oyster,  clam,  or  other  shells  with  a  drop 
of  HC1,  and  see  whether  there  is  effervescence  ;  or  put  them  into  a  gen.  and 
test  the  gas.  (e)  Obtain  CaCl2  from  the  C  O2  gen.  (f )  Test  that  salt  for  Cl 
(Exp.  90).  (g)  For  Ca  (Exp.  74).  (h)  Obtain  CaSO4  from  CaC  08.  (i)  Ca(NO3)2. 


Terms:  Carbonate  of  lime,  quicklime,  slaked  lime,  lime  water,  milk  of 
lime,  sulfate  of  lime. 


37.    CHLOKIN. 

I.  Preparation  from  Hydrochloric  Acid. 

Put  into  a  flask  (or  t.t.)  5g  Mn02  (preferably  granulated)  and 
10CC  H  Cl.  Shake  them  well  together,  apply  gentle  heat,  and  avoid 
inhaling  the  gas,  but  collect  it  by  downward  displacement  in  a  rec. 
loosely  covered  with  paper.  Add  more  HC1  if  it  is  needed.  Ob- 
serve and  describe,  with  equations.  Note  when  the  rec.  is  filled,  to 
avoid  passing  the  gas  into  the  room.  If  accidentally  any  is  inhaled, 
the  antidote  is  vapor  of  alcohol  (inhale  from  a  handkerchief)  ;  or 
NH3  will  do.  State  the  color  of  the  gas,  its  sp.  gr.  compared  with 
air,  its  effect  on  the  nasal  organs. 

II.  Tests  and  Properties, 

(1)  Drop  into  the  rec.  a  piece  of  dry  Turkey-red  cloth  (or  of 
calico),  also  bits  of  printed  and  written  paper.  If  there  is  little 
or  no  effect  add  a  very  little  water,  shake  the  gas,  water,  cloth  and 
paper  well  together,  and  note  the  effect.  Which  bleach  better,  wet 
or  dry  fabrics  ?  (2)  Into  another  rec.  of  Cl  (dried  if  possible)  file 
a  little  Sb  (or  stibnite,  Sb2S3).  Describe  the  result  and  give  an 
equation.  Is  this  a  case  of  ordinary  combustion  ?  Pass  some  Cl 
from  the  gen.  into  sols,  of  :  (3)  AgN03 ;  (4)  Pb(N03)2 ;  (5)  H2S. 

Supplementary.  —  (a)  Put  into  a  small  beaker  5s  bleaching  powder,  CaCl20, 
set  this  into  a  larger  rec.  or  beaker,  putting  into  this  last  the  substance  to  be 
bleached.  Cover  the  large  rec.  with  pasteboard,  through  which  passes  a  thistle- 
tube  into  the  smaller.  Pour  through  the  thistle- tube  5CC  dilute  H2SO4  (half 
H2O  and  half  acid).  Add  more,  if  needed,  (b)  Mix  a  gram  of  fine  NaCl  with 
a  gram  of  Mn02,  add  in  a  t.t.  2CC  H2O  and  3cc  H2SO4,  and  heat.  Observe  any 
gas.  Test  it  with  N  H3,  or  otherwise,  (c)  Dip  some  unglazed  paper  into  oil  of 
turpentine,  CioHie,  in  an  e.d.;  warm  it  by  holding  the  paper  near  a  flame  for 
an  instant  (or  heat  the  turpentine  in  an  e.d.  over  a  waterbath),  but  do  not  set  it 
on  fire.  Then  at  once  thrust  the  paper  into  a  rec.  of  Cl.  Explain  the  combustion 
and  describe  all  you  saw,  giving  the  equation.  Clean  the  rec.  with  naphtha  or 
petroleum. 

Terms :   Bleaching,  bleaching  powder,  calcium  hypochlorite,  chlorid  of  lime. 


38.    EUCHLORIN,  C1O2,  CL 

I.  Preparation. 

Drop  into  a  t.t.  3  or  4  crystals  of  K  C103.  Add  a  few  drops 
H  01,  heat  for  an  instant  and  then  add  5  or  10CC  H20. 

II.  Tests. 

(1)  Observe  carefully  the  action,  noting  the  color  and  odor 
(cautiously),  and  give  equation.  (2)  To  2CC  indigo  sol.  in  a  t.t.  add 
a  little  euchlorin.  Is  the  color  discharged  ?  Test  in  the  same  way 
sols,  of  (3)  litmus  and  of  (4)  cochineal.  (5)  Try  K2O207  sol.  (a 
mineral  pigment ;  the  other  three  are  vegetable  or  animal  coloring 
matters).  What  do  you  conclude  from  this  ?  (6)  Very  cautiously 
add  2  or  3  drops  of  H2S  04  to  2  or  3  small  crystals'of  K  C103  in 
a  t.t.  at  arm's  length  from  the  operator,  then  fill  the  t.t.  with  H20. 
Describe  the  result  with  equation.  (7)  Try  to  bleach  a  piece  of 
Turkey-red  cloth  or  calico  by  putting  it  into  some  euchlorin  and 
leaving  it  a  few  minutes. 

Supplementary.  —  (a)  Try  to  bleach  K  Mn04  sol.  Will  euchlorin  dis. : 
(b)  Au  ?  (c)  Zn  ?  (d)  Cu  ?  Try  its  action  on  sols,  of :  (e)  AgN03 ; 
(f)Pb(N03)2;  (g)HgN03. 

Terms :  Euchlorin,  oxids  of  chlorin,  detonation. 


y  /v 


39.    BKOMIN  AND  BROMIDS. 

I.  Preparation  of  Br. 

(1)  Make  some  starch  paste  by  pulverizing  a  piece  of  starch  not 
larger  than  a  pea,  adding  10CC  H20  and  boiling  several  minutes  in 
a  t.t.;  cool  it  and  dil.  with  10CC  H20,  shaking  it  well.  Boil  again  if 
necessary.  [Save  part  of  this  for  subsequent  exps.]  (2)  Mix  1  or 
2  crystals  of  KBr  with  an  equal  quantity  of  Mn02,  put  them  into 
a  t.t.  and  add  a  few  drops  H2S04.  Heat  the  mixture  and  observe 
carefully.  Write  the  equation,  and  explain  the  action. 

H,  Tests. 

(1)  Dip  a  strip  of  paper  into  the  starch  paste,  wind  it  around 
the  end  of  a  s.r.  and  carefully  put  it  into  the  t.t.,  so  as  not  to  touch 
the  sides.  Then  heat  the  mixture  in  the  t.t.  Observe  the  effect  of 
the  Br  on  the  starch.  The  product  is  supposed  to  be  starch  bromid. 
Avoid  getting  much  Br  into  the  air  in  the  room,  or  inhaling  it. 
Alcohol  vapor,  or  ammonia,  is  the  antidote,  as  for  Cl.  Do  you 
notice  any  effect  of  Br  vapor  on  the  eyes  ?  (2)  To  a  sol.  of  KBr 
add  a  few  drops  of  euchlorin.  Describe  and  explain,  stating  which 
is  the  more  stable  or  stronger  cpd.,  KBr  or  KC1,  and  how  this  exp. 
shows  it.  (3)  Add  to  a  few  drops  of  starch  paste  10CC  H20,  shake 
it  well,  add  a  few  drops  of  KBr  sol.  and  one  drop  of  euchlorin. 
Describe  and  explain. 

Supplementary.  —  Liquid  Br  should  be  examined,  (a)  Try  the  action  of 
Br  on  a  mixture  of  starch  paste  and  KI  sol.  Try  the  action  of  H2S04  on  (b)  a 
few  drops  of  K  Br  sol. ,  also  on  (c)  a  crystal  of  K  Br.  (d)  Pour  a  little  Br  vapor 
from  a  gen.  into  5CC  of  KI  sol.  (e)  Put  a  drop  of  CS2  into  a  t.t.  with  a  few 
drops  of  KBr  sol.,  then  add  a  few  drops  of  euchlorin  and  shake  it.  Notice  the 
color  of  the  C  S2  at  the  bottom  of  the  tube.  The  Br  was  set  free  and  dis.  by 
the  CS2. 


40.    IODIN  AND  IODIDS. 

I,  Preparation  of  I. 

Prepare  I  like  Br  in  the  previous  exp.,  using  KI  instead  of 
KBr.  Notice  the  difference  in  its  action,  color,  state,  etc.,  and  give 
a  full  description  with  equation. 

II.  Properties  and  Tests. 

(1)  Make  the  same  tests  with  starch  as  in  Exp.  39,  noting  the 
different  results.  (2)  Warm  1  or  2  crystals  of  I  in  a  dry  t.t. 
Notice  the  color  of  vapor,  and  its  relative  weight  (pour  a  little  into 
a  dry  e.d.).  (3)  While  warming  the  tube  hold  a  s.r.  half  way  down 
the  t.t.  Look  for  a  sublimate  on  the  rod  and  on  the  sides  of  the 
tube,  examining  carefully  its  form,  luster,  and  color.  (4)  Put  into 
a  small  t.t.  1  or  2  crystals  of  I,  add  3  or  4CC  of  alcohol,  C2H5OH, 
and  warm  a  minute.  Explain,  then  (5)  add  a  drop  of  this  with  a 
s.r.  to  a  drop  of  starch  sol.  shaken  up  with  10  or  15CC  of  H20.  Ob- 
serve the  color  of  the  product  (starch  iodid),  and  boil  it  a  moment 
to  see  whether  the  color  disappears.  If  not,  too  much  I  was  used. 
When  it  is  cool  (hold  the  tube  under  a  jet  of  water)  observe  again. 

Supplementary.  —  (a)  See  whether  a  crystal  of  I  will  dis.  in  H2O.  To  de- 
termine this  apply  the  starch  test,  (b)  To  5  or  10CC  H2O  add  a  drop  or  two  of 
CS2  and  of  KI  sol.  (examine),  then  one  drop  of  euchlorin.  Shake  well,  let 
stand,  and  note  the  color  of  the  C  S2  globule,  (c)  Test  the  solubility  of  I  in 
ether  (C2H5)2O,  keeping  the  latter  away  from  the  flame,  (d)  Obtain  crystals 
by  letting  the  ether  sol.  evaporate,  (e)  To  10CC  H2O  add  a  few  drops  KI  sol. 
and  a  few  drops  of  starch  paste.  Shake  well  together  and  note  the  color.  Now 
add  one  drop  of  euchlorin  (Exp.  38).  If  too  much  euchlorin  is  added  the  sol. 
becomes  green  or  black  (ppt.  of  I).  Describe  the  coloration  and  explain  fully, 
(f)  Repeat  (e)  of  Exp.  39  with  KI  sol. 

Terms :   Sublimation,  sublime,  crystal,  tincture. 


41.    EXPERIMENTS  WITH  SULFUR. 

I.  Crystallization, 

Into  a  small  beaker  or  large  t.t.  put  10  or  15g  S,  and  slowly 
melt  it  over  a  lamp  (using  sand  bath  or  asbestos),  not  allowing  it 
to  become  darker  than  amber-color.  When  it  is  melted  remove  the 
lamp,  leave  the  beaker  in  position  (or  hold  the  t.t.  in  the  hand), 
and  when  crystals  begin  to  shoot  across  the  surface,  pour  the  liquid 
S  remaining  into  water  in  an  e.d.  Explain. 

Loosen  the  S  by  pouring  round  the  edges  a  little  H  N  03.  Warm 
if  necessary,  when  the  mass  may  be  removed  with  a  thin  knife-blade. 

II.  Allotropy. 

Put  10g  S  into  a  t.t.  and  slowly  melt  it.  Notice  the  yellow  color, 
and  see  that  the  liquid  (now  above  100°)  is  very  thin.  Slowly 
continue  to  heat  it  till  it  becomes  black.  Note  that  it  is  now  very 
thick  and  can  scarcely  be  poured  (about  200°).  Apply  more  heat 
till  it  grows  thin  again  (above  300°).  Now  heat  to  boiling  (over 
400°),  note  the  color  of  the  vapor,  and  any  sublimate  on  the  t.t. 
If  it  takes  fire  (S  burns  at  230°),  cover  the  mouth  of  the  tube 
with  paper  or  cardboard  for  a  minute.  Pour  the  S  into  an  e.d.  of 
water.  Pull  it  and  note  its  elasticity.  Is  it  now  crystalline,  or 
amorphous  ?  See  whether  it  afterward  changes.  Clean  the  t.t.  as 
before. 

III.  Solubility. 

Place  in  an  e.d.  -Jg  pulverized  brimstone  and  cover  it  with  CS2 
(avoid  a  flame,  as  CS2  is  explosively  inflammable).  See  whether 
any  dissolves.  Let  it  stand  till  the  C  S2  has  evaporated,  watching 
it  meantime.  Describe  fully  the  phenomena. 

Supplementary.  —  (a)  Try  to  dis,  a  little  S  in  ether,  (C2H5)2O,  and  let 'it 
evaporate.  Is  S  soluble  in  H20  ?  (b)  Grind  together  on  a  brick  with,  a  pestle 
or  other  implement,  not  over  a  half  gram  of  S  and  K  C103.  (c)  Make  gunpowder 
by  mixing  intimately  very  fine  KNO3,  C,  and  S  (a  small  quantity  of  each).  Pile 
the  mixture  on  a  brick  and  cautiously  set  it  on  fire.  If  this  reaction  is  correct, 
in  what  proportion  should  the  constituents  be  mixed  :2KNO3  +  3C  +  S  =  K2S 
+3  CO2  +  2  N  ?  (d)  Obtain  flowers  of  S  by  sublimation  and  see  whether  they 
are  crystalline  or  globular  (use  compound  microscope),  (e)  Add  HC1  to  a  sol. 
of  Na-jS^s  and  look  for  a  S  ppt.  (f )  Obtain  S  O2  from  S,  also  from  H2S  04. 
(g)  Try  to  bleach  with  it  a  green  leaf  or  a  blue  petal. 

Terms :  allotropy,  allotropic,  fusion,  crystalline,  globular,  amorphous. 


42.    HYDROGEN   SULFLD. 

Preparation  and  Tests. 

(1)  Put  into  a  gen.  (rec.  or  t.t.)  5*FeS,  10CC  H20,  and  5ec  HC1 

(or  H2S04).    Adjust  a  d.t.,  having  the 
joints  perfectly  tight,  and  pass  the  gas 
for  a  minute  or  two  into  5CC  H20  in  an- 
other t.t.  or  beaker  (Fig.  36).   Note  the 
odor.      Can  you   determine  whether 
e  gas  is  soluble  in  H20  ?     (2)  See 
whether  the  sol.  is  acid,  alkaline,  or 
Fig-36.  neutral.     With  a  s.r.  put   a   drop  of 

H2S  sol.  on  bright  coins  of  (3)  Ag  and  (4)  Cu.  State  the  effect, 
products,  reactions.  (5)  Put  a  drop  of  Pb(C2H302)2  sol.  on  paper  and 
pass  the  gas  over  it  from  the  tube  of  the  generator.  Describe  the 
effect  (this  is  the  characteristic  test  for  H2S)  and  write  the  equation. 
Is  there  any  other  way  in  which  you  would  recognize  this  gas  ? 

(6)  Try  the  combustibility  of  H2S,  using  a  philosopher's  lamp. 

(7)  If   it   burns,  hold   a   glass   tube   or   a   crayon   in  the   flame. 
Explain. 

II.  As  a  Reagent. 

Add  a  little  H2S  sol.  to  5CC  of  each  of  the  following  sols.,  describe 
the  results,  write  equations  where  necessary,  and  explain  why  there 
is  no  effect  in  certain  cases :  (1)  HgCl2,  (2)  CuCl2,  (3)  BaCl2, 
(4)  CaCl2.  (5)  Next  mix  3  or  4CC  CuCl2  sol.  and  the  same 
quantity  of  BaCl2  sol.,  add  H2S  sol.,  shake  it  well  and  filter.  What 
is  the  residue  and  what  does  the  filtrate  contain?  (6)  Now  to  the 
filtrate  add  a  sol.  of  Na2C03.  State  the  effect,  give  the  reaction, 
and  explain  how  the  Cu  and  the  Ba  have  been  separated. 

III.  Test  for  Sulfids. 

To  a  little  Na2S  or  CaS  add  H2S04.  If  any  gas  arises  (heat  if 
necessary)  try  the  Pb(C2H302)2  test. 

Supplementary.  —  See  whether  you  can  separate  (a)  Cu  from  Ca ;  (b)  Ca 
from  Hg ;  (c)  Hg  from  Ba ;  (d)  Fe  from  Cu.  How  are  some  insol.  sulfids  made  ? 
(e)  Test  FeS  for  a  sulfid  ?  What  sulfids  are  insoluble  ? 

Terms :  sulfuretted  hydrogen,  sugar  of  lead,  sulfid. 


43.     PHOSPHORUS. 

Caution:  Phosphorus  must  be  handled  with  forceps,  as  the 
burns  from  it  heal  very  slowly,  and  all  experiments  with  it  must 
be  done  cautiously.  None  should  be  dropped  upon  the  floor,  nor 
left  upon  the  apparatus,  and  all  must  finally  be  burned.  C  S2  must 
be  kept  away  from  the  flame. 

I.  Spontaneous  Combustion, 

(1)  Into  an  e.d.  put  10  or  20CC  of  C  S2  (for  a  class)  and  drop  into 
it  3  or  4  small  pieces  of  P.  Notice  the  odor  of  CS2  and  whether 
the  P  dissolves  in  it.  Also  observe  the  color  and  luster  of  newly 
cut  P.  (2)  Dip  a  piece  of  unglazed  paper  into  the  sol.,  then  place 
it  on  the  ring  of  a  r.s.  till  it  is  dry,  looking  out  for  any  action.  If 
such  occurs  state  fully  ivhat  has  caused  it  and  whether  it  is  a  case 
of  ordinary  combustion. 

II,  Combustion  under  Water. 

Put  into  a  large  t.t.  4  or  5  crystals  of  KC103,  cover  it  with  H20 
and  add  a  small  piece  of  P.  Rest  the  t.t.  in  a  rec.,  and  then  slowly 
add  2  or  3CC  H2S  O4  through  a  thistle  tube  which  reaches  to  the  P 
and  K  C103.  Account  for  the  phenomena.  What  color  is  the  liquid, 
and  what  is  the  cause  of  it?  HKS04,  HC104,  C102  and  H20 
are  formed.  Write  the  equation  for  forming  them,  and  for  the 
combustion.  What  compound  of  P  is  finally  formed  ? 

Supplementary.  —  (a)  Put  a  small  piece  of  P  into  a  dry  e.d.  in  a  dark  room, 
observe,  and  explain  the  result,  (b)  Put  a  piece  of  P  on  a  dry- plate  or  e.d.,  set 
it  on  fire  and  at  once  cover  with  a  dry  inverted  rec.  When  the  fumes  settle  add 
a  very  little  water.  Test  the  product  with  litmus,  (c)  Cover  a  small  piece  of 
P  with  bone  black  in  a  plate,  and  leave  for  some  time.  If  no  action  ensues 
burn  the  P  before  leaving  the  Exp. 

Terms :  spontaneous  combustion,  phosphorescence. 


%  w  > :      r  <3 

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44.    ARSENIC. 

I.  Marsh's  Test. 

Caution :  AsH3  is  a  deadly  poison,  and  must  not  be  inhaled. 
If  the  H  is  ignited  before  introducing  the  As  compound  there  is 
little  danger. 

Prepare  a  hydrogen  gen.,  with  or  without  a  CaCl2  drying  attach- 
ment, and  with  lamp  tube  (Fig.  37,  or  model).  Put  in  a  few  pieces 

of  arsenic-free  Zn,  some  distilled 
water,  and  C.P.  HC1.  After  a  few 
minutes  test  the  H  gas  (Exp.  13) 
before  lighting,  and  when  no  sharp 
explosion  occurs  light  the  gas,  and 
observe  the  color  of  the  flame.  Test 
37-  for  As  by  holding  an  e.d.  over  the 

flame.  Now  pour  through  the  thistle  tube  1  or  2CC  of  a  sol.  that 
may  be  supposed  to  contain  some  cpd.  of  As.  This  sol.  may  be 
obtained  either  by  dissolving  HNa2As03  in  H20  with  a  little  HC1, 
or  by  immersing  in  HC1  a  small  piece  of  green  paper  tag  from 
which  any  As  that  may  be  present  will  dis.  as  AsCl3.  Note  any 
change  in  the  color  of  the  flame;  hold  an  e.d.  or  other  cold  body 
in  the  flame  and  look  for  a  deposit ;  put  a  Bunsen  flame  under  the 
drawn  out  tube  (Fig.  37)  and  look  for  a  sublimate  just  beyond. 
Absence  of  a  sublimate  in  either  'case  indicates  absence  of  As. 
Explain  fully,  writing  all  equations. 

II.  Reinsch's  Test. 

Into  a  sol.  of  an  As  salt  (obtained  by  HC1  as  above)  in  a  beaker 
or  e.d.  put  a  small  strip  of  bright  Cu  foil  and  heat  for  a  few 
minutes.  Notice  that  the  foil  changes  color.  After  a  few  minutes 
remove  it,  dry  it  by  carefully  pressing  between  folds  of  blotting 
paper,  cut  it  into  strips,  and  put  them  into  a  t.t. ;  heat  the  latter. 
Notice  the  vapor  and  sublimate,  As406,  on  the  tube.  This  sublimate 
may  be  examined  under  the  microscope  after  first  breaking  the 
tube.  Explain  all  results,  using  equations. 

Supplementary.  —  (a)  Reduce  As4O6  as  follows  :  Mix  intimately  a  bit  of  it 
not  larger  than  a  wheat  grain  with  as  much  powdered  charcoal,  put  the  mixture 
into  a  small  t.t.  or  i.t.  and  heat  strongly.  Note  the  vapor,  color,  sublimate, 
(b)  Make  Scheele's  green  by  mixing  sols,  of  CuCl2  and  HNa^AsOs  (or  other  sol. 
cpds.)  and  having  them  nearly  neutral,  (c)  Try  the  effect  on  these  mixtures  of 
(d)  excess  of  HC1,  (e)  excess  of  NH4OH.  (f)  See  whether  As406  is  very  soluble 
in  H20  by  putting  a  very  little  into  a  t.t.  and  heating  with  H20.  (g)  Heat  a  little 
powdered  arsenopyrite,  FeAsS,  in  a  t.t.  and  note  the  odor,  (h)  Test  some 
wall  paper,  or  colored  silk,  for  As. 


45.    COMPOUNDS   OF  BORON. 

I.  Boric  Acid. 

Put  5*  of  Na2B407  into  a  t.t.,  add  10CC  of  dil.  H2S04  and  boil 
till  it  is  clear,  adding  more  water  if  necessary.  Then  cool  it  by 
holding  the  tube  under  a  jet  of  water,  keeping  watch  for  crystals. 
When  it  is  cool  pour  off  the  supernatant  liquid  and  rinse  the 
crystals  once  or  twice  with  water  to  remove  the  H2S  04,  then  put 
them  into  an  e.d.  Add  a  very  little  water,  and  when  the  crystals 
have  dissolved  dip  into  the  sol.  a  piece  of  turmeric  paper,  which 
should  then  be  dried  and  the  color  noted.  Describe  fully  the 
results. 

II.  Borax  Beads. 

Make  a  loop  in  the  end  of  a  Pt  wire  (which  is  welded  into  a 

short  glass  tube,  Fig.  38) .   Moisten 

c«=s=s=^ o  the  loop  end  and  dip  it  into  some 

powdered  borax,  Na2B407.     Now 
heat  it,  using  the  mouth  blowpipe, 

dipping  it  again  into  the  borax  if  more  is  wanted,  and  heating  till 
a  clear  transparent  bead  is  obtained.  Describe  and  explain  the 
phenomena.  Beads  may  be  colored  as  follows :  If  blue  is  wanted 
dip  the  clear  bead  into  a  very  dil.  sol.  of  some  Co  salt,  as  CoCl2,  and 
fuse  again.  -(If  too  much  Co  is  used  it  will  look  dark.)  For  other 
colors  v.  Table  G.  Detach  the  beads  by  suddenly  jerking  the  Pt 
wire  while  the  bead  is  fused.  Save  the  beads,  and  label  them, 
stating  the  coloring  material. 

Supplementary.  —  (a)  See  whether  H3B  03  is  more,  or  less,  soluble  in  hot 
water  than  in  cold,  (b)  Make  a  bead  of  H3B  03  if  possible,  (c)  Stir  a  little 
H3B  O3  in  an  e.d.  with  a  few  drops  of  CgHsOH.  Then  take  some  of  the  mixture 
on  a  short  glass  tube  and  hold  it  in  a  Bunsen  flame,  noting  the  color  imparted 
to  the  latter,  (d)  Try  the  same  with  Na^O?,  (e)  then  with  Na2B4O7  to  which 
has  been  added  a  few  drops  of  H2S04. 

Terms:  borax  bead,  flux. 


46.    COMPOUNDS  OF  SILICON. 

I.  Silicic  Acid  and  Silica. 

Pour  a  few  cubic  centimeters  of  water  glass,  H4Si04,  into  an  e.d. 
and  add  a  little  H  Cl.  Note  the  phenomena,  describe  the  result  and 
write  the  equation.  Pour  off  the  extra  HC1  and  rinse  the  residue, 
H4Si04,  2  or  3  times  with  H20.  Now  heat  it  over  a  Bunsen  flame, 
with  stirring.  This  leaves  Si02.  Write  the  equation,  and  note  how 
the  product  feels  when  rolled  between  the  fingers.  Is  silicic  acid 
made  differently  from  other  acids  ?  Pulverize  (in  a  mortar  if 
necessary)  some  of  the  Si02  obtained,  to  use  in  the  following. 

II.  Silicates  by  Solution. 

Make  a  strong  sol.  of  NaO  H  (or  K  0  H)  and  add  to  it  some  of 
the  Si02  obtained  above,  very  finely  powdered.  Heat  and  stir 
the  mixture  for  some  time.  See  whether  the  Si02  dissolves,  and 
write  an  equation. 

III.  Silicates  by  Fusion,  Glass. 

Make  a  small  mixture  of  equal  parts  of  powdered  Na2C03 
and  K2C03  and  fuse  the  mixture  into  a  bead  as  in  the  case  of  borax. 
Note  that  the  bead  is  opaque  when  cold.  Is  it  so  when  hot  ?  Dip 
this  bead  when  hot  into  a  little  Si02  powdered  very  finely,  then 
heat  again  more  strongly  in  the  hottest  part  of  the  flame.  If  it  is 
not  transparent  when  cold,  dip  it  again  into  the  Si02  and  heat  more 
strongly  than  before.  See  whether  it  now  resembles  glass.  Describe 
all  phenomena  and  write  the  equations.  Colors  may  be  obtained  as 
in  borax  beads,  Table  G. 

Supplementary.  —  (a)  Try  to  dis.  finely  powdered  Si02  in  a  strong  sol.  of 
Na2CO3,  boiling  the  mixture,  (b)  Try  to  fuse  Si02  in  a  borax  bead. 

Terms:  fusible,  infusible,  fusion,  transparent,  opaque,  silica,  silicate,  glass, 
water  glass. 


47.    OXIDATION  AND  REDUCTION. 

I.  Oxidation. 

(1)  Into  each  of  two  tubes  put  5CC  FeS04  sol.  (freshly  dissolved). 

To  one  of  these  add  a  few  drops  HN03  and  boil  a  minute,  then  cool. 

To  each  of  the  tubes  add  5CC  NaO  H  sol.  (or  NH4OH).  Observe  the 

color  effects,  explain  their  causes,  and  give  equations  for  the  ppts. 

Explain  the  action  of  H]ST03. 

(2)  Put  a  small  fragment  of  Pb  on  a  piece 
of  charcoal,  slightly  hollowed  out  with  the 
handle  of  the  forceps.  Fit  a  metallic  tube  to 
a  Bunsen  burner,  and  with  a  mouth  blow-pipe 
blow  the  oxidizing  flame  (outer)  strongly  and 
steadily  against  the  Pb  for  4  or  5  minutes 
(Fig.  39).  What  first  takes  place?  As  you 
stop  blowing,  notice  the  yellow  vapor  that 
escapes  from  the  globule  of  Pb  :  also  the  yellow 

a,  red^Snfflame.       coating  of  Pb  0  on  the  charcoal.    Explain  fully, 

b,  oxidizing  flame.       using  equations. 

II.  Reduction. 

(1)  Pour  a  little  FeCl3  sol.  into  two  tubes.     Pass  S  02  gas,  or 
H,  from  a  gen.  into  one  of  these  for  a  few  minutes.     Next  add 
NH4OH   to   each.       Compare    the    products   and  explain,   with 
equations.     What  action  has  the  S02ortheH?     Try  the  action 
of  Zn  and  H,  or  of  Zn  alone. 

(2)  Put  £g  PbO  on  a  piece  of  charcoal  hollowed  out  as  before. 
With  the  blow-pipe  blow  the  reducing  flame  (inner)  steadily  against 
it  for  some  time,  or  until  a  metallic  globule  is  obtained.     What  is 
it?     Explain  fully,  with  equation.     See  whether  the  globule  is 
sectile  (can  be  cut)  or  malleable  (can  be  flattened  by  pressure). 
Extinguish  the  fire,  if  the  coal  still  glows,  with  a  drop  of  water. 

Supplementary.  —  Notice  that  the  action  of  the  flames  here  is  like  that  of 
oxidizing  and  reducing  agents  generally,  (a)  Experiment  with  other  metals  and 
oxids.  (b)  See  whether  Fe(OH)2  or  Fe(OH)3  tends  to  change  to  the  other  on 
standing.  Which  is  the  more  stable  cpd.  ?  (c)  Try  sols,  of  FeS  04  and  FeCl3 
in  the  same  way.  (d)  Try  to  oxidize  FeSO4  sol.  with  a  little  euchlorine. 
(e)  Oxidize  HgN03  with  HNO3.  (f)  Try  to  reduce  K2Cr2O7  sol.  to  CrCl3  with 
a  little  HC1,  C2H5OH  and  heat.  Note  the  change  in  color,  also  test  by  Exp.  48. 
Are  these  oxidizing,  or  reducing  agents:  (g)  KC103,  (h)  KNO3,  (i)  C,  (j)  Cu  ? 
(k)  Pulverize  about  a  gram  of  K  N  O3  and  mix  it  with  a  like  quantity  of  fine 
charcoal.  Put  into  a  dry  i.t.  and  heat.  (1)  Try  KNO3  and  S  in  the  same  way. 

Terms:  Oxidation,  reduction,  oxidizing  agent,  reducing  agent,  oxidizing 
flame,  reducing  flame. 


48.    LEAD,  Pb". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.    Ppt.  PbCl2  (v,  Ag,  Hg'). 

To  Pb(N03)2  sol.  add  HC1,  filter 
(test  fil.),  wash,  reject  washing 
(and  fil.  if  no  more  PbCl2  falls). 

(1)  PbCl2 

white 

2.    Dis.    PbCl2  in   hot   H20.    (v.   Ag, 

Hg')- 

Pour  on  res.  (1)  boiling  H20  from 
t.t.     Save  fil. 
Repeat  this  several  times. 

(a)  PbCl2 

3.   Final  test  for  Pb. 

To  first  filtrate  (a)  add  K2Cr207 
sol.  (or  K2Cr04). 

(2)  PbCr04 

yellow 

Supplementary.  —  1.  PbCl2  is  somewhat  sol.  in  H20,  hence  traces  of  it  are 
tested  for  in  Grp.  II.  3.  If  there  is  much  free  acid  in  a  sol.  the  K2Cr207  test  is 
not  to  be  relied  on.  H2S  04  should  then  be  used.  What  other  Pb  salt  might  be 
used  for  sol.  (Table  A)  ?  (a)  Allow  some  of  the  hot  water  sol.  of  PbCl2  to  cool 
in  a  t.t.  and  look  for  crystals.  Explain,  (b)  See  which  is  the  stronger  cpd. 
PbCl2  or  PbCr04.  (c)  Make  several  other  final  tests  for  Pb. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENT. 

REMARKS. 

1 

2 

AmOH 
NaOH 

Pb20(OH)2 
Pb(OH)2 

white 
u 

(  NaOH  (ex.), 

With  PbAc2  no  ppt., 
Pb2OAc2  being  sol. 

8 

Am2C03 

Pb3(C03)2(OH)2 

u 

STaOH  (ex.), 

4 

NfeCOa 

Pb3(C08)2(OH)2 

u 

INO 

5 

HC1 

PbCl2 

(i 

]_ 

I20  (boiling) 
FTfll  (sL) 

Re-ppts.,  cryst.,  on  cooling. 

G 

H2S 

PbS 

black 

dil.  HNO.t 

HN03  (str.)  forms  PbS04. 

H2S  +  HX08  ppts.  S. 

7 

Am2S 

PbS 

u 

dil.  HNOs 

HN08  (str.)  forms  PbS04. 

Am2S  +  HX08  ppts.  S. 

8 

KI 

PbI2 

yellow 

H20  boiling 

Re-ppts.,  cryst.,  on  cooling. 

9 

H2S04 

PbS04 

white 

TaOH'(ex  ) 

Dis.by  Na2S2O3  (v.  BaS04). 

10 

K2Cr207 

PbCr04 

yellow 

• 

gaUS 

HC1  changes  ppt.  to  PbCl2. 

11 

Am20x 

PbOx 

white 

WE*^ 

12 

HNa2P04 

Pb3(P04), 

(4 

• 

'JaOH  (ex.), 

13 

KCy 

PbCy2 

U 

KCy  (ex), 

Boiling  re-ppts. 

14 

KiFeCy,, 

Pb^eCy* 

*' 

15 

Zn 

Pb 

metallic 

dil.  HNOs 

Also  Al,  Cd,  Co,  Mg. 

16 

Mb.  } 

Pb 

" 

dil.  HN03 

Yel.  PbO  on  C.C. 

49.    SILVER,  AgT- 


ANALYTICAL    REACTIONS. 


BISECTIONS. 

PPT. 

COLOB. 

SOL. 

1.    Ppt.AgCl(v.  Pb,  HgO 

To  AgN03  sol.  add  HC1,  filter  (test 
fil.),  wash  res.,  reject  fil.  and 
washings. 

(l)AgCl 

white 

2.    Dis.  AgCl  in  NH4OH  (v.  Hg',  Pb). 

To  (1)  add  NH4OH  on  filter,  and 
catch  fil.  in  t.t. 

(a) 
(NH3)3  (AgCl)2 

3.    Be-ppt.  AgCl. 

Cautiously  acidify  (a)  with  HN03 

(2)  AgCl 

white 

Supplementary.  —  1.  Strong  HC1  dis.  AgCl  (and  HgCl  somewhat) ;  hence 
avoid  excess.  2.  In  testing  for  trace  of  Ag,  evap.  NH3  before  adding  HN03. 
3.  Never  add  the  latter  in  large  excess.  AgCl  is  not  re-ppd.  by  H  Cl  except  in 
cone.  sols,  (a)  Sep.  Ag  from  Pb.  Are  most  salts  of  Ag  soluble  (Table  A)  ? 
Can  these  exist  together  in  sol:  (b)  AgN03  and  HgCl2  ?  (c)  AgNO3  and  CuCl2  ? 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENT. 

EEMABKS. 

1 

AmOH 

brown 

(AmOH£x.,, 

AgOH  is  not  known. 

(  HAc',H2S04  3> 

2 

NaOH 

'  ' 

n 

3 

Am2C03 

Ag2C03 

white 

Am.oCOs  (ex.), 
AmOH,HN03 

4 

TflTflrfifO 

** 

u 

5 
6 

HCl 
H2S 

AgCl 
Ag2S 

black 

|AmOH,KCy, 

(Na^Os 

boilingHNO, 

HN03  re-ppts.    Light  re- 
duces to  Ag2Cl,  violet, 
black. 

7 

Am,S 

" 

u 

« 

8 

KBr 

AgBr 

white 

AmOH  (si.) 

9 

El 

Agl 

(yellow- 
jwhite 

KI  (ex.) 

Insol.  in  AmOH. 

10 

K2CrsOT 

Ag,Cr04 

(dark 

(AmOH, 
\HN08 

HCl  changes  it  to  AgCl. 

11 

Am20x 

Ag20x 

white 

AmOH 

12 

HNa2P04 

Ag3P04 

yellow 

(  AmOH, 
(HNOs 

13 

KCy 

AgCy 

white 

KCy  (ex.) 

14 

Ag4FeCVrt 

{yellow- 

Boiling  gives  metallic  Ag. 

• 

j  white 

15 

Zn 

Ag 

gray 

dil.  HNO< 

Also  Bi,  Cu,  Fe,  Hg,  Pb. 

16 

Na2C03,  ) 
B.B.C.C.  ) 

Ag 

it 

HNOs 

Metallic  globule. 

50.    MERCURY  (ous),  Hg'. 
ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.   Ppt.  HgCl  (v.  Ag,  Pb). 
ToHgN03  sol.  add  HC1,  filter  (test 
fil.),  wash,  reject  fil.  and  wash- 
ings. 

(l)HgCl 

white 

2.  AmOE  on  HgCl  (v.  Ag,  Pb). 
On  (1)  pour  a  little  AmOH,  wash 
and  reject  washings. 

(2)NH2Hg2Cl 

black 

3.  Dis.  NH2Hg2Cl  in  aqua  regia. 
On  (2)  pour  a  few  drops  aqua  regia, 
save  fil. 

(a)  HgCl2 

4.  Ee-ppt.Hgd. 

Dilute  (a),  add  SnCl2  sol. 

(3)  HgCl 
Hg 

white 
gray 

Supplementary.  —  1.  Hg',  not  Hg",  must  be  used  as  HgCl2  is  sol.  3.  The 
smallest  quantity  of  aqua  regia  that  will  dis.  the  ppt.  must  be  used.  4.  SnCl2 
sol.  must  be  newly  prepared,  and  with  plenty  of  HC1,  or  it  will  oxidize  to  SnCU 
and  Sn2O  C12.  (a)  Sep.  Hg'  from  Ag.  (b)  Hg/  from  Pb.  Explain  action  of 
SnCl2  on  HgCl2.  (c)  Can  HgN  O3  and  CuCl2  exist  in  sol.  together  ?  (d)  HgN  03 
andCdC!2? 

GENERAL  REACTIONS. 


RK-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

NHjHg2N03 

black 

HN03,aq.reg. 

2 

NaOH 

Hg20 

(  brown- 
]  black 

«          « 

Hg2O  (instable)  =  Hg  + 
HgO.  HgOH  not  known. 

3 

Am,C03 

NH,Hg2N03 

black 

Acids, 

4 

NazCOs 

HgzCOs 

gray 

Forms  black  Hg20  on  boil- 

ing. 

5 

HC1 

HgCl 

white 

HNO, 

With  AmOH  =  NH2Hg2Cl 

(black). 

6 

H2S 

Hg8S 

black 

aq.reg. 

Hg2S  (instable)  -  HgS+  Hg 

7 

Am2S 

« 

1  1 

« 

8 

El 

Hgl 

(yellow- 
]  green 

KI  (ex). 

Ex.  forms  HgI2(sol.)  +  Hg. 
Acids  decompose  it. 

9 

H2S04 

Hg2S04 

white 

HNOs 

In  strong  sol.  only. 

10 

K2Cr207 

Hg2CrO* 

yellow 

HN03 

11 

AmoOx 

Hg20x 

white 

« 

12 

HNa2F04 

HgsPO* 

« 

« 

13 

ZCy 

HgCy2+  Hg 

gray 

H20 

Hg  ppd. 

14 

K.FeCyB 

Hg4FeCyfi 

white 

HNOs 

15 

Zn. 

Hg 

gray 

HNOs,  aq.reg. 

Also  Al,  Bi,  Cd,  Cu,  Mg. 
Sn  amalgamates  with  M. 

1  A 

Na,C08,  ) 

He- 

a 

«           « 

Heat  in  tube  with  Na2C03 

lo 

B.B.C.C.  ) 

**•& 

+  C,  and  Hg  sublimes. 

51.    GROUP  I.  -  Pb",  Ag ,  Hg . 

ANALYTICAL  REACTIONS. 
PPT. 


DIRECTIONS. 


SOL. 


1.  Fpt.  PbCl2,  AgCl,  HgCl. 

Sat.  sol.  with  HC1,  filter,  wash, 
reject  washings. 

2.  Sep.  Pb  from  Ag.Hg. 

On  (1)  pour  boiling  H20.  Repeat 
till  last  fil.  gives  no  ppt.  with 
K2Cr2O7  sol. 

3.  Final  test  for  Pb. 

To  (a)  add  K2Cr2O7  sol.  (or 
K2Cr2O4). 

4.  Sep.  Ag.  from  Hg. 

On  (2)  pour  warm  AmOH  two  or 
three  times. 

5.  Final  test  for  Ag. 

Acidify  (b)  with  HN03. 

6.  Dis.  NH2Hg2Cl. 

To  (4)  add  very  little  aqua  regia. 

7.  Final  test  for  Hg. 

To  (c)  add  SnCl2  sol. 


(l)PbCl2,AgCl,HgCl 

(2)  AgCl,  HgCl 

(3)  PbCr04 

(4)  NHoHg2Cl 

(5)  AgCl 

(6)  HgCl,  Hg 


(a)  PbCl2 


(b)(NH3)3(AgCl)£ 


(c)  HgCl, 


Supplementary.  —  1.  Avoid  large  excess  of  HC1,  as  it  may  interfere  with 
the  ppts.  of  H2S,  Grp.  II-  AgCl  is  less  sol.  than  HgCl,  HgCl  than  PbCl2.  H  Cl 
may  give  a  ppt.  outside  of  Group  I  as  follows :  of  S,  if  a  sulfid  or  thiosulfate  is 
present ;  of  BaCl2  (sat.  sol.)  which  is  sol.  in  H2O  but  insol.  in  strong  HC1 ;  of 
BiOCl,  SbOCl,  Sn2OCl2,  from  sols,  acidified  with  other  acids  than  HC1  (these 
are  sol.  in  excess  of  HC1);  of  As2S3,  Sb2S3,  SnS2,  AgCy,  XiCy2,  H4Si04, 
H3B03,  Zn(OH)2,  A1(OH)3,  from  an  alk.  sol.  In  any  of  the  above  cases  if  an 
appreciable  ppt.  falls,  insol.  in  H20  or  HC1,  dis.  and  analyze  separately. 
2.  PbCl2  should  all  be  removed  by  successive  additions  of  hot  H20  (test  the  last 
fil.  with  a  drop  of  AgNO3  sol.),  as  NH4OH  changes  it  to  white  insol.  Pb2OCl2, 
some  of  which  appears  in  the  fil.  H  N  O3  however  dis.  it.  It  may  be  better  to 
boil  the  liquid  which  holds  the  first  ppt.  before  filtering,  then  filter  and  test  the 
fil.  for  Pb.  3.  What  other  reagent  might  be  used  here  ?  4.  Why  is  not  AgN03 
formed  ?  I  have  a  white  powder  which  is  PbCl2,  HgCl,  or  AgCl.  What 
reagent  will  determine  which  it  is  ? 


52.    MERCURY  (ic),  Hgr'. 
ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.   Ppt.  HgS(v.Pb,Bi,Cd,Cu,As,Sn,Sb). 

Sat.  sol.  with  H2S  gas,  filter  (test 

fil.),  wash. 

(1)  HgS 

black 

2.   HgS  insol.  in  Am2S,  (v.  As,  Sn,  Sb). 

To  (1)  in  e.d.  add  Am2Sx,  stir,  boil,  1 

decant,  wash. 

(2)  HgS 

u 

3.  HgS  insol.  in  dil.  HN03  (v.Pb,Bi,Cd, 

Cu). 

Cover  (2)  with  dil.  HNO3,  boil  a 

minute,  decant. 

(3)  HgS 

u 

4.   Dis.  HgS  in  aqua  regia  (v.  Hg'). 

• 

To  (3)  add  little  aqua  regia,  stir, 

boil  if  necessary. 

(S) 

(a)  HgCl2 

5.  Ppt.  HgCl  and  Hg  with  SnCl2  (v.  Hg', 

Sn"). 

Boil  (a)  to  expel  all  Cl,  add  SnCl2 

sol. 

(4)  HgCl 

white 

Hg 

gray 

Supplementary.  —  1.  Hg"  salts  often  give  with  H2S  a  ppt.  first  white,  then 
yellow,  red,  brown,  black.  Double  salts.,  e.g.  HgCl2(HgS)2  are  first  formed. 
3.  Strong  HN03  may  convert  HgS  into  Hg(N08)2(HgS)2,  white,  insoluble  ; 
hence  test  a  white  res.  for  Hg.  4.  In  dis.  HgS  use  the  smallest  quantity  of  aqua 
regia  (usually  only  a  few  drops).  The  sol.  may  afterwards  be  diluted.  5.  SnClj 
sol.  is  pearly,  and  must  not  be  confounded  with  a  Hg  ppt.  How  detect  HgN  03  in 
a  mixture  with  Hg(N03)2?  Hg(N03)2  in  presence  of  HgNO3?  Explain  the 
action  of  SnCl2  on  HgCl2.  Is  HgS  sol.  in  strong  H  N03  ?  Why  is  Hg"  not  put 
into  Group  I  ? 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

I 

AmOH 

NH2HgCl 

white 

AmOH,  HC1 

Hg(N03)2  gives  NHg2N08. 

2 

NaOH 

HgO 

y  el.  -red 

HN03 

Hg(OH)2  not  known. 

3 

Am2C03 

NH2HgCl 

white 

AmOH,  HC1 

4 

NfeCOs 

(HgO)3HgC03 

(var.) 

C    red 
j  white 

Forms  HgO  on  boiling. 

5 

SnCl; 

HgCl,  Hg 

gray 

HN03,aq.reg. 

6 

H2S 

HgS 

black 

aqua  regia 

May  be  first  white,  then 

7 

Am2S 

(i 

a 

« 

red,  brown,  black. 

8 

KBr 

HgBr2 

white 

hot  H20 

0 

El 

HgI2 

red 

1  HgCl2 
\  KI  (ex.),  HC1 

10 

K2Cr207 

HgCr04 

orange 

HNOs 

11 

Am:0x 

HgOx 

white 

dil.  HN03 

With  HgCl2  no  ppt.  forms. 

12 

HNazPO* 

Hg3(P04)j 

(i 

acids,  Am.  salts 

13 

KCy 

HgCy2 

it 

KCy  (ex.) 

14 

K4FeCy6 

Hg2FeCy6 

K 

On  stand,  becomes  Pruss.  blue. 

15 

Zn 

Hg 

gray 

Forms  amalgam  with  the  metal 

1  /> 

Na2C03    \ 

TT-_ 

u 

(v.  Exp.  50). 

16  B.B.C.C.J 

Hg 

53.    L.EAD,  Pb". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  PbS  (v.  Hg",  Bi,  Cd,  Cu,  As, 
Sn,  Sb). 

Sat.  sol.  with  H2S,  filter  (testfil.), 
wash. 

2.   PbS  insol.  in  Am2Sx  (v.  As,  Sn,  Sb). 

(1)  PbS 

(  brown- 
(  black 

To  (1)  in  e.d.  add  Am2Sx,  warm, 
decant,  wash. 

(2)  PbS 

u 

3.   Dis.  PbS  in  HN03  (v.  Kg"). 

Boil  (2)  with  dil.  HN03,   evap., 
add  H20. 

(a)  Pb(N03)2 

4.  Ppt.  PbS04  (v.  Bi,  Cd,  Cu). 

To  (a)  add  dil.  H2S04+C2H6OH, 
and  shake  it. 

(3)  PbS04 

white 

Supplementary.  —  1.  Pb  sometimes  gives  colored  ppts.  at  first,  like  Hg",  if 
much  HC1  is  present.  If  there  is  much  mineral  acid,  it  must  be  diluted  or 
partly  neutralized  before  H2S  will  give  a  ppt.  3.  Strong  HNO3  oxidizes  PbS  to 
PbSO4,  and  dil.  acid  does  so  somewhat.  Some  PbSO4  dis.  in  HN03,  and  some 
may  be  left  with  HgS.  Test  the  latter  with  boiling  AmAc  sol.,  filter  and  add 
HAc  +  K2Cr207  sol.  Before  adding  H2SO4  all  HN03  should  be  expelled  by 
evaporation,  (a)  Sep.  Hg"  from  Pb.  Test  the  relative  solubility  in  water  of 
(b)  PbCl2,  (c)  PbS,  (d)  PbSO4.  Can  these  salts  exist  together  in  a  sol.: 
(e)  Pb(NO3)2  +  MgS04  ?  (f)  Pb(NO3)2  +  Na2CrO4  ?  (g)  Pb(NO3)2  +  NaCl  ? 
Explain.  Exp.  48  gives  General  Reactions  for  Pb. 


54.    BISMUTH,  Ei'". 

ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  Bi2S3  (v.  Hg,  Pb,  Cd,  Cu,  As, 
Sb,  Sn). 
Sat.  sol.  with  H2S,  filter,  wash. 

2.  Bi2S3  insol.  in  Am2Sx  (v.  As,  Sn,  Sb). 
To  (1)  add  Am2Sx. 

(1)  Bi2S3 
(2)  Bi2S3 

(  brown- 
j  black 

u 

3.  Dis.  Bi2S3  in  HN03  (v.  Hg.). 
To  (2)  add  dil.  HNO3,  boil  a  min- 
ute, filter. 

(S) 

(a)  Bi(N03)3 

4.  Bi  not  ppt.  by  H2S04  (v.  Pb). 
To  (a)  add  few  drops  H2S04. 

(b)  Bi(N03)3 

5.  Final  test  for  Bi  (v.  Cd,  Cu). 
To  (b)  add  excess  AmOH,  shake, 
let  stand. 

(3)  Bi(OH)3 

white 

Supplementary.  — 1.  Diluting  an  acid  sol.  of  Bi  may  ppt.  BiOCl,  BiON03, 
etc.,  but  H2S  changes  these  to  Bi2S8.  5.  NH4OH  must  be  added  in  excess, 
otherwise  Bi  will  not  ppt.  here,  but  with  Cd  (v.  Group  II,  A),  (a)  Pour  a  few 
drops  of  the  BiCl3  sol.  into  a  t.t.  of  H2O.  BiCl3  reacts  with  H2O,  and  forms 
insoluble  BiOCl  (v.  Sb).  (b)  Test  Bi(NO3)3  sol.  in  the  same  way.  BiNO3(OH)2 
(variable)  is  ppd.  Name  the  ppts.  Try  to  dis.  them  with  acids:  (c)  HC1, 
(d)  HNO3,  (e)  HAc.  Most  salts  of  Bi  react  with  H2O.  This  confirmatory  test 
may  be  tried  in  analysis.  Ppt.  (f)  a  Bi  salt  and  (g)  a  Pb  salt  (in  2  tubes)  with 
K2Cr2O7  sol.,  and  test  solubility  of  each  in  NaOH  sol.  What  would  this 


reaction  distinguish  ?    Now  add 
(i)  Bi  from  Pb  ;  (j)  Bi  from  Ag. 


SnCl2  sol.  to  each,     (h)  Sep.  Bi  from  Hg"; 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Bi  OH*;          white 

Acids 

Boil,  gives  Bi2O3  (yel.-wh.). 

2 

NaOH 

<( 

" 

« 

No.  ppt.  with  H2Tr  or  H3Ci. 

3 

AmgCOs 

Bi202C03 

" 

« 

4 

Na2COs 

ti 

u 

d 

5 

SnClo 

BiO 

black 

With  excess  NaOH  (T.  Cl). 

6 

Ht8 

BiA 

u 

HN03(dil.) 

Insol.  in  Am2Sx. 

7 

Am2S 

« 

t( 

d 

u        u          u 

KI 

\  (BiOD 

(dark 

HC1 

/  Bil  . 

(brown 

9 

H20 

BiOCl 

white 

HC1 

Others  give  basic  salt. 

10 
11 

K2Cr207j 
or  Z2Cr04  ) 

Bi20(Cr04)2 

yellow 

HNO 

Insol.  in  NaOH  (v.  Pb). 

12 

Am20x 

Bi20xs 

white 

HN03 

13 

HN^POi 

BiP04 

" 

HC1 

Insol.  in  HNO3  or  HAc. 

14 

KCy 

Bi(OH)3 

" 

Acids 

Insol.  in  excess  KCy., 

15 

K4FeCy« 

BuFeCyis 

(  yellow- 
1  white 

HNO 

Reppts.  on  boiling. 

16 

Zn 

Bi 

spongy 

" 

Also  Cu,  Fe,  Pb,  Sn. 

17 

B.B.C.C.  i 

Bi 

dark 

" 

Incrustation  yellow. 

i 

55.     CAI>MIUM,  Cd". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  CdS  (v.  Hg,  Pb,  Bi,  Cu,  As,  Sb, 
Sn). 
Sat.  sol.  with  H2S;  filter,  wash. 

(1)  CdS 

yellow 

2.  CdS  insol.  in  Am2Sx  (v.  As,  Sb,  Sn). 
To  (1)  add  Am2Sx  in  e.d.;  stir. 

(2)  CdS 

yellow 

3.  Dis.  CdS  in  HN03  (v.  Hg). 
Boil  (2)  a  minute  with  dil.  HNO3. 
Filter  if  necessary. 

(S) 

(a)  Cd(N03)2 

4.  Cd  not  ppd.  by  H2S04  (v.  Pb). 
To  (a)  add  a  drop   or  two  dil. 
H2S04. 

(b)  Cd(N03)2 

5.  Cd(OH)2  dis.  by  excess  AmOH  (v.  Bi). 
To  (b)  add  excess.  AmOH. 

(c) 
(NH3)2CdO(AmN03)2 

6.  Cd  not  ppd.  by  KCy  (v.  Cu). 
To  (c)  add  little  KCy  sol. 

(d)  (KCy)2CdCy2 

7.  Ke-ppt.  CdS  (v.  Cu). 
Sat.  (d)  with  H2S. 

(3)  CdS 

yellow 

Supplementary.  —  1.  If  a  large  excess  of  acid  is  present  the  sol.  must  be 
diluted  before  H2S  will  act.  (a)  Sep.  Cd  from  Bi.  (b)  Sep.  Cd  from  Hg". 
(c)  Sep.  Cd  from  Pb.  What  sol.  salts,  if  any,  of  Cd  have  the  corresponding  salts 
of  Cu  insol. ,  or  vice  versa  (v.  Table  A)  ?  (e)  Devise  any  method  of  separating 
Cd  from  Cu,  dependent  upon  this,  and  try  it. 

GENERAL   REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Cd(OH)2 

white 

AmOH(ex) 

2 

NaOH 

it 

« 

Acids 

Insol.  in  excess. 

3 

Am2C03 

CdC03 

« 

4 

NfeCOs 

« 

u 

« 

Free  Am  prevents,  ppt. 

5 

H2S 

CdS 

yellow 

i  Hot,  dil. 
iHNOs 

6 

Am2S 

u 

n 

« 

7 

K2Cr2OT 

CdCrO* 

It 

HNO. 

In  concentrated  sols.  only. 

8 

Am20x 

CdOx 

white 

Acids  (si.) 

9 

HNa^ 

Cd3(P04)2 

u 

Acids 

10 

KCy 

CdCy2 

u 

KCy  (ex.) 

Re-ppd.  by  H2S. 

11 

K^FeCyB 

Cd2FeCyB 

u 

(HC1 
1  AmOH 

12 

KaFeCyr, 

Cd3FeaCy12 

yellow 

i  AmOH 
IHC1 

13 

Zn 

Cd 

gray 

Also  Al,  Mg. 

14 

Na.COs     ) 
B.B.C.C.  \ 

CdO 

(  brown- 
!  yellow 

Incrustation,  no  globule. 

56.    COPPER,  Cu". 

ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  CuS  (v.  Hg,  Pb,  Bi,  Cd,  As,  Sb, 
Sn). 
Sat.  sol.  with  H2S,  filter,  wash. 

2.  CuS  insol.  in  Am2Sx  (v.  As,  Sb,  Sn). 
To  (1)  add  Arn2Sx  ;  stir. 

3.  Dis.  CuS  in  HN03  (v.  Hg). 
To  (2)  add  dil.  HNO3,  boil  a  min- 
ute, filter  if  necessary. 

(1)  CuS 
(2)  CuS 

(S) 

(  brown- 
I  black 

(  brown- 
l  black 

(a)  Cu(N03)2 

4.  Cu  not  ppd,  by  H2S04  (v.  Pb). 
To  (a)  add  a  drop  or  two  H2SO4. 

(b)  Cu(N03)2 

5.  Cu  salts  sol.  in  excess  AmOH  (v.  Bi). 
To  (b)  add  excess  AmOH. 

(c) 
(NH3)2CuO(AmN03)2 

6.  Action  of  KCy  on  Cu  salts  (v.  Cd.). 
To  (c)  add  KCy  sol.  until  blue 
color  disappears. 

(d)  (KCy)2CuCy.> 

7.  Inaction  of  H2S  on  (KCy)2CuCyo 
(v.  Cd). 
Pass  H2S  into  (d). 

(e)  (KCy)2CuCy.2 

8.  Final  test  for  Cu. 
To  (e)  add  HC1. 

(3)  CuS 

{  brown- 
(  black 

Supplementary.  —  5.  If  the  sol.  does  not  become  blue  on  adding  NH4OH, 
Cu  is  absent.  2.  CuS  dis.  slightly  in  (NH4)2SX.  Neutralizing  such  a  sol.  with 
HC1  gives  a  liver-colored  ppt.  (a)  Sep.  Cu  and  Pb;  (b)  Cu  and  Hg";  (c)  Cu 
and  Bi.  (d)  Can  CuCl2  exist  in  sol.  with  Na^COa  ?  (e)  Cu(NO3)2  and  Na2S  ? 
(f)  CuCl2and  MgSO4? 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Cu(OH)2 

blue 

AmOH  (ex.) 

Unsat.,  pale-blue  basic. 

2 

NaOH 

« 

u 

« 

Boiling  gives  black  CuO. 

3 

Am2C03 

Cu2(OH)2C03 

u 

Am2C03(ex.) 

it                    U                U                  U 

4 

H2S 

CuS 

black 

HNOs,  KCy 

5 

Am2S 

u 

" 

«        d 

6 

KI 

CuI,I 

yel.-wh. 

KI(ex.) 

7 

K2Cr04 

Cu2Cr04(OH)2 

red-br. 

8 

Am20x 

CuOx 

(  blue- 
i  white 

j  M.  acids 

i  Am20x(ex.) 

9 

HNa2P04 

HCuP04 

U   ' 

Acids 

Cu  (ex.)  gives  Cu3(PO4)2. 

10 

KCy 

CuCy2 

gr.-yel. 

KCy  (ex.) 

H2S  has  no  effect  on  KCy. 

11 

Cu2FeCy6 

red-br. 

AmOH 

Dil.  sol.  gives  red  color. 

12 

KBr+H62S04 

None. 

red 

A  drop  or  two  of  each. 

13 

Zn 

Cu 

" 

HNOs 

Also  Al,  Bi,  Fe,  Ni,  Pb,  Sn. 

14 

B.B.C.C.  i 

" 

u 

" 

No  incrustation. 

57.    GROUP  II,  A.-Ug  9  Pb,  Bi,  Cd,  Cu. 

ANALYTICAL   PEACTIONS. 


DIRECTIONS. 


PPT. 


SOL. 


1.  Ppt.  HgS,  PbS,  Bi.2S;j,  CdS,  CuS 

{v?As,~Sn,  Sb). 
Sat.  sol.  with  H2S  gas,  filter, 
test  filtrate,  wash  residue 
until    washings    give    no 
ppt.  with  a  drop  AgNO3. 

2.  Separate  Hg  from  Pb,  Bi,  Cd, 

Cu. 

To  (1)  add  little  dil.  HN03, 
boil  a  minute,  decant,  leave 
residue. 

3.  Dis.  HgS  in  aqua  regia. 

To  (2)  add  a  few  drops  aqua 
regia,  stir,  warm  if  neces- 
sary. 

4.  Final  test  for  Hg  (v.  Hg",  Sn). 

Boil  to  expel  all  free  Cl,  add 
SnCl2  sol. 

5.  Sep.  Pb  from  Bi,  Cd,  Cu. 

Expel  all  HNO3  from  (a),  add 
little  dil.  H2S04+C2H5OH, 
shake,  let  stand,  filter,  test 
fil. 

6.  Sep.  Bi  from  Cd,  Cu. 

To  (c)  add  AmOH,  shake, 
let  stand,  filter. 

7.  Sep.  Cd  from  Cu. 

To  (d)  add  KCy  sol.  until 
any  blue  color  disappears, 
then  sat.  (e)  with  H2S. 

8.  Final  test  for  Cu. 

Acidify  (f)  with  HC1. 


(1)  HgS,  PbS, 
Bi2S3,  CdS,  CuS 


(2)  HgS  (S) 

(S) 

(3)  HgCl,  Hg 

(4)  PbS04 

(5)  Bi(OH)3 

(6)  CdS 

(7)  CuS 


(a) 

Pb(N03)2,  Bi(N03)3 
Cd(N03)2l  Cu(N03)2 


(b)  HgCl2 


(c)  Bi(N03)3 
Cd(N03)2 
Cu(N03)2 

(d) 

(NH3)2CdO(AmN03)2 
(NH3)2CuO(AmN03)2 

(e)  (KCy)2CdCy2 
(KCy)2CuCy2 

(f)  (KCy)2CuCy2 


Supplementary.  —  1.  Acidulate  the  original  sol.  with  HC1  (not  HNO3, 
which,  like  other  oxidizing  agents,  decomposes  H2S).  Unless  the  sol.  is  acid, 
Co,  Ni,  Zn  are  liable  to  ppt.  if  present.  If  too  acid,  Cd,  Pb,  etc.,  will  not  ppt. 
If  no  ppt.  falls,  dil.  the  sol.  1.  Be  sure  the  sol.  is  sat.  with  H2S ;  to  ascertain 
this  test  the  fil.  2.  A  black  res.  may  not  be  HgS,  but  S  with  enclosed  particles 
of  PbS,  Bi2S3,  CuS.  Hence  confirm  by  SnCl2.  5.  Test  a  small  part  of  the  sol. 
for  Pb  at  first.  6.  Excess  of  AinO  H  must  be  used  to  ppt.  all  the  Bi  (which 
otherwise  may  appear  in  the  final  Cd  test)  and  to  dis.  Cu(OH)2  and  Cd(OH)2  at 
first  formed.  Bi  may  be  confirmed  by  dis.  ppt.  in  a  few  drops  of  HC1,  evapo- 
rating free  acid  and  adding  to  H20.  6.  If  the  color  is  not  blue  on  adding 
AmO  H  no  appreciable  Cu  is  present.  Unless  previously  removed  Pb  will  ppt. 
with  AmOH.  7.  The  final  Cd  ppt.  must  be  yellow.  If  not,  some  of  the  other 
metals  have  failed  to  ppt.  at  the  right  place,  and  will  appear  here. 

As,  Sn,  Sb  —  Group  II,  B  —  are  omitted  here  for  brevity.  They  are  ppd. 
by  H2S,  and  may  be  separated  from  the  whole  of  Group  II  by  dissolving  in 
Am2Sx  (v.  Exp.  61).  If  Group  I  metals  were  not  removed  by  HC1,  would  they 
ppt.  with  Group  II  (test  each  with  H2S)  ? 


58.    ARSENIC,  As'". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  As2S3  (v.  Group  II,  A;  Sn,  Sb). 
Sat.  sol.  with  H2S,  filter  (test  fil.), 
wash. 

(1)  As2S3 

yellow 

2.  As2S3  insol.  in  HC1  (v.  Sn,  Sb). 
Cover  (1)  with  HC1,  boil  a  min- 
ute, filter,  wash. 

(2)  As2S3 

yellow 

3.  Dis.  As2S3  in  Am2Sx. 
To  (2)  add  Am2Sx,  boil,  filter   if 
necessary. 

(S) 

(a)  Am3AsS3 

4.  Re-ppt.  As2S3. 
Cautiously  acidify  (a)  with  HC1. 

(3)  As2S3,(S) 

yellow 

Supplementary.  —  The  original  sol.  should  be  acidified  with  H  Cl.  (a)  Try 
a  neutral  sol.  with  H2S,  also  (b)  an  alkaline.  H2S  acts  very  slowly  on  Asv,  but 
more  rapidly  when  hot  than  when  cold,  ppg.  As2S3+ S.  Test  (c)  an  acid,  (d)  a 
neutral,  (e)  an  alkaline  sol.  of  As  salts  with  a  sol.  of  a  Cu  salt.  What  2  yellow 
ppte.  formed  by  H2S  ?  (f)  Test  the  solubility  of  each  in  Am2Sx. 

GENERAL  REACTIONS. 


RB-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

fAmfVH 

1 

AgNO, 

AgsAsOs 

yellow 

1  AJliUXl 

<  dil.  HCl 
LAmCl 

Asv  (neutral)  +  AgNO3  = 
Ag3AsO4  (red-brown). 

2 

H,S 

ASaS., 

(  lemon- 
/  yellow 

fAm2COs 
4  Am2Sx 
LNaOH 

Re-ppd.  by  HCl. 

3 

AmcS 

« 

d 

« 

4 

CnS04 

HCuAsOs 

green 

(AmOH 
I  ail.  acids 

Scheele's  green  (Paris  green). 

5 

KMnO* 

Decolorized. 

« 

f!n  A  /*• 

(  CuCXAsoOv* 

u 

(AmOH 

Schweinfurt  green. 

U 

vQAUl 

iCuACj 

land  acids 

Paris  green. 

7 

Cu 

As 

gray 

aq.  reg, 

Heated  with  HCl  (Reinsch's 

test). 

8 

H  (nascent) 

AsH3  (ga«) 

Burns  with  pale-white  flame. 

Deposits  As  on  porcelain. 

AsH3  very  poisonous 

(Marsh's  test). 

9 

Na,C08+KCy 

As 

gray 

HCl 

Sublimed  if  heated  dry. 

10 

*C  (heated) 

« 

u 

« 

Garlic  odor. 

11 

lAmCPAmOH 
1    +MgS04 

AmMgAs04 

white 

« 

For  Asv  only. 

12 

Am3MoO, 

AmAs'MoO;, 

yellow 

« 

Composition    uncertain    (v. 

M8P04). 

59.    TIN,  Sn' . 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  SnS  (v.  Group  II,  A  ;  As,  Sb). 
Sat.  sol.  with  H2S,  filter,  wash. 

(1)  SnS 

chocolate 

2.  Dis.  SnS  in  HC1  (v.  As). 
To   (1)    add   HC1,  boil,  filter  if 
necessary. 

(S) 

(a)  SnCl2 

3.  Hg  test  for  Sn. 
To  (a)  add  HgCl2  sol. 

(2)  HgCl, 
Hg 

white 
gray 

Supplementary. — SnCl2  sol.  should  be  freshly  prepared,  and  both  Sn  and 
H  Cl  left  in  the  sol.  Otherwise  SnCl4  and  Sn2O  C12  are  formed.  Sniv  with  H2S 
gives  yellow  SnS2,  sol.  in  Am2Sx,  or  Am2CO3.  (a)  Try  to  dis.  Sn  in  HN03 
(strong  and  dil.).  Try  to  dis.  part  of  the  res.  in  (b)  HC1,  part  in  (c)  aqua  regia. 
What  metals  have  no  nitrates?  Which  of  the  following  can  exist  in  sol. 
together  ?  (d)  SnCl2  and  HgCl ;  (e)  SnCl4  and  HgCl ;  (f)  SnCl4  and  HgCl2. 
(g)  Change  SnCl2  to  SnCl4 ;  (h)  SnCl4  to  SnCl2.  Give  proof  of  the  change  in 
both  cases,  (i)  Sep.  Sn  from  As.  (j)  Can  SnCl2  and  AgN03  exist  in  sol. 
together  ?  (k)  SnCl2  and  PbCl2  ? 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Sn(OH)2 

white 

NaOH 

Ppt.  from  Sniv  is  SnO(OH)2, 

white. 

2 

NaOH 

" 

" 

ii 

Boiling  gives  SnO.    Boiling 

NaOH+HoTr  gives   Sn 

(black). 

3 

Am.CO 

" 

it 

" 

Insol.  in  excess  (v.  Sb"'). 

4 

Na;CO 

« 

" 

« 

"            '•            " 

5 

HgCl2 

HgCl+Hg 

}white, 

If  dil.  HgCl,  if  strong  Hg. 

{WoATT 

{Normal  Am2S  does  not 

6 

H2S 

SnS 

brown 

il  d  wil 

HC1 

dis.  SnS. 
If  Sniv  is  present,  ppt.  is 

XX  vl 

SnS2  (yellow). 

7 

El 

SnI2 

yellow 

HC1,  NaOH 

In  neutral,  concentr.  sol. 

8 

Am20x 

SnOx 

white 

HC1 

9 

HN^PO, 

SH3(P04)2 

" 

Acids 

10 

ECy 

Sn(OH)2 

" 

HC1,  NaOH 

HCy   (very    poisonous)   is 

evolved. 

11 

E4FeCy6 

Sn2FeCyB 

'« 

12 

HN03,  Cl 

Oxidizes  Sn"  to  Sniv. 

13 

0  or  H,0 

Sn2OCl- 

white 

HC1 

SnCl4  also  formed  and  dis- 

solved.  Sn  and  HC1  add- 

ed retard  action. 

14 

Zn 

Sn 

igray, 
I  spongy 

«       * 

Also  Al,  Cd,  Mg. 

Na2COs    ) 

Use    excess    Na2C03    and 

15 

B.B.C.C.  ) 

little  KCy. 

6O.    ANTIMONY,  Sb'". 
ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  Sb2S3  (v.  Group  II,  A-,  As,  Sn). 
Sat.  sol.  with  H2S,  filter,  wash. 

2.  Dis.  Sb2S3  in  HC1  (v.  As). 
To   (1)  add   HC1,  boil,   filter  if 
necessary. 

3.  Inaction  of  HgCl2  on  SbCls  (v.  Sn). 
Divide  (a),  to  half  add  HgCl2  sol. 

4.  Ke-ppt.  Sb2S3. 
Dilute  other  half  (a),  add  H2S. 

(1)  Sb2S3 
Sb2S3 

orange 
« 

(a)  SbCl:; 
(b)  SbCl3 

Supplementary. — Sb2S8  will  not  ppt.  from  too  acid  or  too  alkaline  sols., 
and  only  imperfectly  from  neutral.  SbCl3  is  insol.  in  H2O,  reacting  with  it  to 
form  insol.  SbOCl  (which  H2S  changes  to  Sb2S3).  It  should  be  acidulated  with 
HC1.  Try  to  dis.  Sb  in  HNO3.  If  not  sol.,  test  the  res.  (a)  with  HC1,  (b)  with 
aqua  regia.  (c)  Add  HgCl2  sol.  to  SbCl3  sol.  Explain,  (d)  Apply  the  "spot 
test,"  i.e.  Marsh's  test  (Exp.  44),  to  Sb.  (e)  Sep.  Sb  from  Sn ;  (f)  Sb  from  As. 
Would  you  be  likely  to  find  SbCl3  in  sol.  with  the  first  group  metals  ?  With  a 
purely  aqueous  sol.  of  Group  II,  A  ? 

GENERAL  REACTIONS. 


KE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

BM, 

white 

(Hot  NaOH  (ex.), 
I  HC1 

Sol.  should  be  slight- 
ly acid. 

2 

NaOH 

(( 

tt 

«        « 

"        "        " 

3 

Am2CO: 

f( 

u 

«        « 

(1                  U                  U 

4" 

(HC1, 

u            u            u 

AftilAJa 

1  hot  Am2C03 

5 

H20 

SbOCl  (var.) 

u 

Acids 

Part  only  ppts. 

fAm2Sx, 

6 

Hs8 

Sb2S3 

orange 

j  NaOH, 

IhotHCl 

7 

Am2S 

u 

u 

i< 

If  too  acid  or  too  al- 

kaline, no  ppt. 

8 

El 

no  ppt. 

yellow 

Sbv  ppts.  I. 

9 

Am20x 

Sb(NHs)3Ox3 

white 

Ppts.  slowly. 

10 

ECy 

uncertain 

" 

11 

EtFeCye 

u 

u 

Insol.  in  acids. 

12 

Zn 

Sb 

black 

aqua  regia 

Also  Bi,  Cu,  Mg,  Fe, 

Sn. 

rMetallic,  brittle, 

13 

Na,CO,    1 
B.B.C.C.  i 

" 

" 

aqua  regia 

1  white     incrust., 
1  green  flame,  white 
I  fumes  (Sb2O3). 

61.    GROUP  II,  B.  —  As,  Sn,  Sb. 

ANALYTICAL   REACTIONS. 


DIRECTIONS. 


PPT. 


SOL. 


1.  Ppt.  As2S3,  SnS,  Sb.>S3  (v.  Group  II, 

^)- 
Sat.  sol.  with  H2S,  filter,  wash. 

2.  Sep.  Sn  and  Sb  from  As. 

Warm  (1)  in  e.d.  some  time  with 
HC1,  decant  on  filter. 

3.  Dis.  As2S3. 

To  (2)  add  Am2Sx,  boil,  filter  if 
necessary. 

4.  Final  test  for  As. 

Cautiously  acidify  (b)  with  HC1. 

5.  Final  test  for  Sn. 

Divide  (a),  to  half  add  HgCl2 
sol. 

6.  Final  test  for  Sb. 

Dilute  other  half  (a),  add  H2S. 


(1)  As2S3,  SnS,  Sb2S3 

(2)  As2S3  (S) 

(S) 

(3)  As2S3  (S) 

(4)  HgCl,  Hg. 

(5)  Sb.2S;> 


(a)  SnCl2,  SbCl3 

(b)  Am3AsS, 


Supplementary.  — 1.  If  there  is  very  much  HC1  in  the  sol.,  Sb  and  Sn  may 
not  ppt.  To  determine  this,  dilute  a  little  of  the  sol.,  and  test  with  H2S. 
2.  The  sol.  should  be  warmed  with  H  Cl  in  excess  some  time,  not  boiled,  or  As 
will  go  into  solution.  As2S3  may  be  dis.  by  a  sat.  sol.  of  Am2CO3  (made 
without  AmOH),  warmed,  and  sep.  from  Sb  and  Sn ;  then  ppt.  As2S3  with 
HC1  (cautiously).  3.  If  no  appreciable  res.  is  left  in  2  except  S,  omit  3.  6.  If 
Sb  is  present,  an  orange  ppt.  will  appear  first,  followed  later  (if  Sn  is  also  there) 
by  chocolate  SnS.  Metals  of  Group  II,  J3,  are  sep.  from  those  of  Group  II,  J., 
by  dis.  the  sulfids  of  the  former  in  Am2Sx  (not  Am2S).  A  white  ppt. ,  on  adding 
HC1  is  liable  to  be  S.  (a)  Sep.  SbCl3  from  CuCl2;  (b)  SnCl2  from  BiCl3. 


62.    IRON  (ic),  Fe'". 
ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  Fe(OH)3  (v.  Cr,  Al). 

To  sol.  add  AmCl  sol.  ,  AmOH,  warm, 

filter,  wash  res. 

(1)  Fe(OH)3 

red 
I  brown 

2.  Dis.  Fe(OH)3  in  HC1  (v.  Cr,  Al). 

To  (1)  in  e.d.  add  dil.  HC1,  stir. 

(a)  FeCl3 

3.  Be-ppt.  Fe(OH)3  with  NaOH  (v.  Cr,  Al). 
To  (a)  add  excess  NaOH  sol. 

(2)  Fe(OH)3 

(red 
1  brown 

Supplementary.  —To  reduce  Fe'"  to  Fe"  v.  Exp.  47.  To  oxidize  Fe"  to 
Fe'"  v.  Exp.  47.  Test  FeCl3  sol.  (Fe'")  in  t.t.  with  a  few  drops  of  (a)  K4FeCy6, 
(b)  K3FeCy6,  (c)  KSCy,  (d)  NaOH.  (e)  Test  also  FeS04  sol.  (Fe")  with  the 
same  reagents,  and  tabulate  results.  Then  state  what  will  distinguish  Fe" 
from  Fe'".  (f)  Dis.  a  little  Fe  in  dil.  H2SO4,  nearly  evap.,  add  H2O,  and  then 
determine  whether  FeS04  or  Fe2(SO4)3  is  found,  (g)  Dis.  a  little  Fe  in  aqua 
regia,  evap.,  dil.,  test  as  before,  (h)  Test  also  the  product  after  dis.  in  HC1. 
(i)  Sep.  Fe'"  from  Cu";  (j)  Fe"  from  Bi'".  (It  is  better  to  oxidize  Fe"  to  Fe'" 
before  separation.)  (k)  Can  a  sol.  contain  both  FeCl3  and  HgNO3  ?  (1)  FeS04 
and  Cu(NO3)2  ?  (m)  Make  FeP04.  Will  H2S  ppt.  FeS  ?  Fe2S3  is  not  formed 
in  aqueous  analysis. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Fe(OH)3 

(red 
(  brown 

Acids 

Variable  to  Fe202(OH)2. 

2 

NaOH 

« 

a 

it 

U                 .<(                       li 

8 

Am2C03 

it 

it 

it 

a             u                it 

Traces  Fe2(C03)3. 

4 

NaaCOs 

K 

n 

« 

Variable  to  Fe202(OH)2. 

5 

HNaPO* 

FeP04 

white 

M.  acids 

Fe"x  (except  FeAc3)  ppt. 

by  this  and  NaAc  (v. 

M3P04). 

6 

AmaOx 

Fe20x3 

u 

Acids 

7 

KCy 

Fe(OH)3 

|red 
I  brown 

d 

HCy    formed    (very  poi- 
sonous). 

8 

Z4FeCy6 

Fe4FesCy18 

blue 

H2SO* 

Prussian  blue.    NaOH  + 

ppt.  =  Fe(OH)3. 

9 

KsFeCye 

No  action;   distinguishes 

Fe'"  from  Fe". 

10 

KSCy 

FeCy3S3 

(  blood- 
ied 

Color  only,  no  ppt. 
Disting.  Fe'"  from  Fe". 

11 

H2S 

S 

white 

Reduces  Fe"'  to  Fe". 

12 

Am,S 

FeS+S 

black 

Acids 

First  reduces  Fe'"  to  Fe". 

13 

j  Tannic  acid 
(    and  galls. 

Fe'"  tannate 

it 

Basis  of  writing  ink. 

14 

NaAc 

Fe2Ac3(OH)3 

red 

15 

(  SO,,  H8S 
1  Zn,  SnCl2 

Reduce  Fe'"  to  Fe". 

63.    IRON,  Fe". 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AuiOH 

Fe(OH)2 

(green 
i  black 

(  AmCl  (si.), 
(  Acids 

White,  if  pure.  Oxidizes 
to  Fe(OH)3,  red-brown. 

2 

NaOH 

(C 

a 

u 

u            u            u 

3 

Am2C03 

FeC03 

white 

u 

Oxidizes  to  Fe(OH)3. 

4 

NaoCO; 

« 

u 

" 

11                U                U 

5 

H,S 

FeS 

black 

u 

With  FeAc2  only  a  slight 

ppt. 

6 

Am_>S 

u 

u 

it 

Oxidizes  to  FeO(S04)2. 

7 

Am,0x 

FeOx 

yellow- 
white 

M,  acids 

Kino 

8 

HNa2P04 

HFeP04 

Diue- 
white 

Acids 

Fe3(PO4)2  also  formed. 

9 

KCy 

FeCy2 

yellow- 
red 

KCy  (ex.) 

10 

K4FeCy6 

K2Fe2Cy6 

blue- 
white 

Oxidizes  in  air  to  Prus- 
sian blue. 

11 

K-FeCy, 

Fe3Fe2Cyi2 

blue 

Distinguishes  Fe"  from 

Fe"'. 

12 

KSCy 

no  effect 

a            u            u 

13 

HN03,  KC103 

14 

Cl,  &c. 

Fe'"  (no  ppt.) 

red 

Oxidizes  Fe"  to  Fe'". 

15 

f  Tannic  acid 
i    +  tincture 
I  gaUs 

Fe"  tannate 

(  white  to 
I  black 

Oxidizes  to  Fe'"  tannate 
(black  ink). 

Supplementary.  —  In  the  separation  of  Fe"  it  is  first  oxidized  to  Fe'",  and 
then  tested  as  in  Group  III.  To  ascertain  whether  you  have  a  ferrous  (Fe")  or 
a  ferric  (Fe'")  salt,  test  the  original  sol.  by  the  table  below,  (a)  Prepare  some 
Prussian  blue ;  (b)  Everitt's  salt ;  (c)  Turnbull's  blue ;  (d)  black  ink. 

TESTS  FOR  FERROUS  AND  FERRIC  IRON. 


RE-AGT. 

FE". 

FE"'. 

K4FeCy6 

Z2FeFeCy6  (bluish  white). 
Potassium    ferrous-ferro-cya- 
nid  or  Everitt's  salt. 

Fe4Fe3Cyi8  (deep-blue). 
Ferric-ferro-cyanid  or  Prus- 
sian blue. 

ZsFeCye 

Fe3Fe2Cyi2  (dark-blue). 
Ferrous-ferri-cyanid  or  Turn- 
bull's  blue. 

FeFeCy6  (green  or  brown  color 
only). 
Ferric-f  erri-cy  anid  . 

KSCy 

No  effect. 

Fe(SCy)3  (blood-red  color  only). 
Ferric-sulpho-cyanid. 

KOH 

Fe(OH)2  (white  to  dirty  green). 
Ferrous  hydroxid. 

Fe(OH)8  (red-brown). 
Ferric  hydroxid. 

64.    ALUMINUM,  Al"'. 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  A1(OH)3  (v.  Fe,  Cr). 
To  sol.  add  AmCl  sol.  ,  AmOH, 
boil,  filter. 

(1)  A1(OH)3 

white 

2.  Dis.  A1(OH)3  in  HC1  (v.  Fe,  Cr). 
To  (1)  add  dil.  HC1,  stir. 

(a)  A1C13 

3.  Dis.  A1(OH)3  in  NaOH  (v.  Fe,  Cr,  Zn). 
To  (a)  add  excess,  strong  NaOH 
sol.,  shake. 

(b)  Na2Al204 

4.  A1(OH)3  insol.  in  AmOH. 

Acidify   (b)  with  HC1,   add 
AmOH. 

(2)  A1(OH)3 

u 

Supplementary.  —  3.  NaO  H  sol.  must  be  in  excess,  and  strong  enough  to  dis. 
the  A1(OH)3  first  formed,  (a)  Sep.  Fe  from  Al.  (b)  Test  action  of  limited 
NaO  H  sol.  on  Al.  (c)  Is  A12S3  formed  in  aqueous  analysis  [try  H2S  and  Am2S  ; 
a  ppt.  is  A1(OH)3]  ?  (d)  Test  Al'"  and  AmCl  sol.  with  NaOH  sol.  (e)  Now 
ppt.  A1(OH)3  with  AmCl  and  NaOH,  and  try  to  dis.  it  in  excess,  (f)  Sep.  Cu 
and  Al ;  (g)  Bi  and  Al.  (h)  Obtain  A1C13  from  several  cpds.  of  Al,  in  two  or 
three  different  ways,  (i)  Obtain  alum  crystals  by  mixing  sols,  of  sulfates  of  Al 
and  K  (Exp.  5).  Try  to  dis.  Al  in  (j)  HC1,  (k)  HNO3. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

rNaOH(ex.)  forms 

1 

AmOH 

A1(OH)3 

(gray 
(  white 

NaOH,  acids 

I    Na2Al2O4,notre- 
I    ppd.  by  boiling 

I   (v.  Zn). 

f  NaOH  (ex.)  forms 

2 

NaOH 

ti 

u 

u 

^    Na2Al204;  AmCl 

[  re-ppts.  it. 

3 

Am2C03 

u 

Na2C03 

Liberates  CO2. 

4 

Na-COs 

" 

NazCOs  (ex.) 

u            u 

5 

Am,S 

(( 

white 

Acids 

H2S  evolved. 

0 

KJeCye 

uncertain 

it 

7 

HNa,POi 

A1P04 

NaOH,  HC1 

8 

NasStOs 

A1(OH)3+S 

Acids 

S02  liberated. 

TFirst  heat  :  infus. 

9 

|  B.B.C.C7. 

I    +  Co(N03)2 

blue 

Add  a  drop  of 
Co(N03)2     sol., 
I  heat:  blue. 

ii  iff   «r- 

|U 


65.    CHROMIUM  (ic),  Cr"'. 
ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  Cr(OH)3  (v.  Fe,  Al). 
To  sol.  add  AmCl  sol.,  AmOH; 
warm. 

(1)  Cr(OH)3 

green 

2.  Dis.  Cr(OH)3  in  HC1  (v,  Fe,  Al). 
To  (1)  add  dil.  HC1,  stir,  filter  if 
necessary. 

(a)  CrCl3 

3.  Oxidize  Cr'"  to  Crvi. 

Evap.  (a)  almost  to  dryness,  then 
add  1  or  2  crystals  KC103,  and 
evap.    to  dryness  ;    add  H2O, 
filter  if  necessary. 

(b)  K2Cr207 

4.  Action  of  NaOH  on  KoCr_,07. 
To  (b)  add  NaOH  sol. 

(c)  K2Cr04 

5.  Ppt.  PbCr04. 

Acidify  (c)  with  HAc,  add 
Pb(N03)2  sol. 

(2)  PbCr04 

yellow 

Supplementary. — 1.  Cr(OH)3  may  dis.  in  cold  water,  but  re-ppts.  on 
boiling.  3.  Cr"'  must  be  oxidized  to  Cr™,  or  it  will  ppt.  with  NaOH  sol. 
(a)  Sep.  Cr"'  from  AY",  (b)  To  K2Cr207  sol.  add  successive  small  portions  of 
AmOH,  shaking  each  time,  till  the  color  becomes  yellow.  Alkalies  reduce  red 
dichromates  to  yellow  chromates;  acids  have  the  reverse  effect,  (c)  Slowly 
acidify  the  chromate  with  HC1.  (d)  Will  Cr(OH)3  ppt.  from  K2Cr2O7  sol.? 
(e)  Reduce  Crvi  to  Cr'".  (f )  Sep.  Cr'"  and  Fe'" ;  (g)  Cr"'  and  Cd.  (h)  Make 
Cr2(S04)3  from  K2Cr207.  (i)  Make  Cr(NO3)3. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Cr(OH)3 

j  blue- 
\  green 

(  NaOH(ex.) 
1  Acids 

Re-ppt.  by  hot  AmCl  or  by 
boiling. 

2 

NaOH 

'* 

" 

NaOH  (ex.) 

it         a         n         tt 

3 

AmoCO; 

" 

" 

Na2C03  (ex.) 

tt         tt         tt         it 

4 

Na-CO;: 

a 

tt 

u 

tt         it         tt         n 

CO2  formed.     Slight  ppt. 

5 

H2S 

Cr202Cr04 

Reduces  Crvi  to  Cr'"  in  pres- 

ence of  HC1. 

6 

Am2S 

Cr(OH)3 

u 

Acids 

Forms  slowly  if  dilute  ;  H2S 

liberated. 

7 

HNaJ?04 

CrP04 

green 

M.  acids 

8 

H2S04+H202 

undeterm. 

blue 

(C2Hs)aO 

Blue  liquid  rises  to  surface 

with  Crvi  only. 

9 

KCy 

Cr(OH)3 

(  blue- 

NaOH 

HCy  liberated. 

(  green 

10 

KC103,  Cl,  &c, 

Cr'"  oxidized  to  Crvi  (yellow- 

red)  with  heat. 

11 

NazCOg+KClOa 

i  K2Cr04 

yellow 

H20 

Fused  on  Pt  foil. 

12 

Na2C03  (bead) 

green 

V.  Table  G. 

66.    GROUP  III.-Fe,  Al,  Cr. 

SEPARATION. 


DIRECTIONS. 

PPT. 

SOL. 

1.  Ppt.  Fe(OH)3,  A1(OH)3,  Cr(OH)3. 

To  sol.  add  AmCl  sol.,  AmOH, 

(1) 

boil  a  minute,  filter,  wash. 

|  Fe(OH)3,  A1(OH)3, 

(     Cr(OH)3 

2.  Dis.    Fe(OH)3,    A1(OH)3,    Cr(OH)3    in 

HN03. 

(a) 

To  (1)  add  dil.  HNO3. 

(Fe(N03)3,Al(N03)3, 

3.  Oxidize  Cr(N03)3  to  K2Cr207. 

I    Cr(N03)3 

Evap.  (a)  to  dryness;    when  al- 

most evap.  add  1  or  2  small 

crystals  KC1O3.     When  evap. 

dis.  in  H2O  ;   decant  on  filter 

and  add  to  res.   a  few  drops 
HNO3  ;  pour  on  same  filter. 

(Fe(N03)3,Al(N03)3, 

i    KoCr207 

4.  Sep.  Fe  from  Al  and  Cr. 

To  (b)  add  excess  strong  NaOH 

(e) 

sol.,  shake,  filter. 

(2)  Fe(OH)3 

Na.:AL04,  K.2Cr04 

5.  Sep.  Al  from  Cr. 

Acidify  (c)  with  HC1,  add  AmOH, 

filter. 

(3)  A1(OH)3 

(d)  K2Cr04 

6.  Final  test  for  Cr. 

Partly  evap.  (d),  dil.,  acidify  with 

HAc,  add  Pb(N03)2  sol. 

(4)  PbCr04 

Supplementary.  —  1.  AmCl  prevents  ppn.  by  AmOH  of  Mg,  Mn,  Zn,  Co,  Ni 
(Fe"  partially),  aids  ppn.  of  Al,  and  does  not  affect  Fe"'  and  Cr.  Considerable 
AmCl  is  needed.  AmO  H  at  first  ppts.  Co,  Ni,  Zn,  if  present,  all  of  which  are 
sol.  in  excess.  If  only  one  of  these  Fe'",  Al,  Cr,  is  present,  the  color  determines 
which.  Cr(OH)3  dis.  in  cold  H20,  but  is  re-ppd.  on  boiling.  Fe"  should  be 
oxidized  to  Fe'"  by  boiling  with  a  few  drops  of  HN03.  H2S  must  all  be 
removed  by  boiling  before  adding  AmO  H,  to  prevent  formation  of  Am2S  and 
ppn.  of  Co,  Ni,  Mn,  Zn.  Cr""  is  reduced  by  H2S  to  Cr'",  and  hence  ppd.  here. 
3.  Cr"'  must  all  be  oxidized  to  Cr™  or  it  will  ppt.  with  Fe.  4.  Fe  should  be 
tested  in  the  original  sol.  for  Fe"  or  Fe'"  by  K4FeCy6,  K3FeCy6,  KSCy. 
6.  NaO  H  dis.  some  SiO2  from  the  containing  bottles,  and  there  may  be  a  ppt. 
of  H4Si04,  similar  to  A1(OH)3,  small  in  quantity  and  sinking  sooner  than 
A1(OH)3.  6.  A  white  ppt.  of  PbCl2  will  always  appear  if  no  Cr  is  present. 
The  yellow  color  alone  indicates  Cr. 


67.    COBALT,  Co". 

ANALYTICAL  REACTIONS. 


BISECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  CoS  (v.  Ni,  Mn,  Zn). 
To  sol.  add  AmCl  sol.,  Am2S, 
shake,  warm,  filter,  wash  res. 
with  hot  H2O,  adding  to  it  a 
few  drops  Ani2S. 

(1)  COS 

black 

2.  CoS  insol.  in  HC1  (v.  Mn,  Zn). 
To  (1)  add  dil.  HC1,  stir,  decant. 

(2)  CoS 

« 

3.  Dis.  CoS  in  aqua  regia  (v.  Ni). 
To  (2)  add  a  few  drops  of  aqua 
reg.,  stir,  filter,  evap.  acid,  dil. 

(S) 

(a)  CoCl2 

4.  Ppt.  K6Co20(N02)i0. 

To  (a)  add  HAc,  KN02  sol. 

(3) 

K6Co.20(N02)10 

yellow 

Supplementary.  —  1.  Am2S  (colorless)  must  be  used,  not  Am2Sx  (yellow). 
2.  CoS  is  sol.  in  strong,  hot  H  Cl,  and  slightly  in  cold,  as  is  NiS.  3.  K6CoO(N  02)io 
is  broken  up  by  alkalies,  or  HC1,  but  not  by  HC2H3O2.  1.  CoS  and  NiS  are 
liable  to  oxidize  to  the  soluble  sulfates  if  exposed  long  to  the  air,  hence  they 
must  be  filtered  and  washed  at  once.  4.  Some  ppt.  may  occur  at  once  in  4,  but 
to  be  sure  all  the  Co  is  thrown  down  24  hours  is  needed,  and  enough  KNO2 
must  be  used.  What  sulfid  in  Group  II  was  sol.  in  aqua  regia  only  ?  Why  is 
not  CoS  ppd.  by  H2S  with  Group  II  ?  (a)  To  Co  salts  add  H2S,  then  AmO  H. 
How  is  Am2S  made  ?  (b)  Make  a  borax  bead  by  fusing  with  the  blow-pipe  a 
little  Na2B4O7  in  the  loop  of  a  Pt.  wire  until  it  becomes  clear.  Dip  this  bead 
into  a  very  weak  sol.  of  CoCl2  and  fuse  again.  The  blue  color  —  if  the  sol.  was 
not  too  strong  —  is  very  characteristic  of  Co.  (c)  Can  AgN  O3  and  CoCl2  exist 
in  sol.  together  ?  Sep.  (d)  Co  and  Cd;  (e)  Co  and  Cr. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Co(OH)2 

red 

J  AmOH  (ex.), 
'  AmCl,  &c. 

f  Blue  bas.  ppt.  first  formed. 
4    On  stand,  forms  Co(OH),. 
i.  Oxidizes  to  Co(OH)3. 

2 

NaOH 

u 

u 

" 

Insol.  in  NaOH  (ex.). 

3 

Am2COs 

Co2OC03 

it 

Am2C03  (ex.) 

Violet  or  blue  by  heating. 

4 

Na2C03 

" 

" 

Insol.  in  excess  Na2CO3. 

6 

Am2S 

CoS 

black 

HN03,aq,reg. 

Oxid.  to  CoSO4,  which  is  sol. 

6 

KN02 

KeCojO(N02>io 

yellow 

HC1 

Ppts.  only  in  pres.  of  HAc. 

7 

KCy 

CoCy2 

br.-wh. 

KCy  (ex.) 

Dist.  from  Ni  by  hot  HC1. 

8 

EUFeCye 

Co2FeCy6 

Grayish  green. 

9 

KaFeCye 

CosTe.Cy. 

J  brown 
(red 

fin  absence  of  Mn",  or  Ni, 
4    AmCl+AmOH+K3FeCy6 
(^  +  Co"  =  blood-red  color  . 

10 

HNa2P04 

HCoPO; 

red 

AmOH,  acids 

11 

Heat  (on  paper) 

blue 

Dehydrated. 

12 

Na2B407  (bead) 

« 

Blue  bead  in  either  flame. 

13 

Cl,Pb02(warm) 

white 

Oxidizes  Co"  to  Co'". 

14 

Zn 

Co 

a 

HC1 

Also  Cd,  Mg. 

15 

B.B.C.C.  i 

" 

u 

Magnetic. 

68.    NICKEL,,  Ni". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  NiS  (v.  Co,  Mn,  Zn). 
To  sol.  add  AmCl,  Am2S,  warm, 
filter  rapidly,  wash  res.  with 
hot  H2O  and  a  few  drops  of 
Am2S. 

(1)  NiS 

black 

2.  NiS  insol.  in  HC1  (v.  Mn,  Zn). 
To  (1)  add  little  dil.   HC1,  stir 
and  decant. 

(2)  NiS 

a 

3.  Dis.  NiS  in  aqua  regia  (v.  Co). 
To  (2)  add  at  once  a  few  drops  of 
aqua  regia,  stir,  filter,  evap. 
acid,  and  dilute. 

(S) 

(a)  NiCLj 

4.  Inaction  of  KN02  on  NiCl  and  HAc. 
To  (a)  add  little  HAc,  KNO2  sol.  ; 
leave  24  hours. 

(b)  NiCl2 

5.  Ppt.  Ni(OH)2. 
To  (b)  add  excess  strong  NaOH 
sol.  ;  boil  if  necessary. 

(3)  Ni(OH)2 

(  apple- 
|  green 

Supplementary.  —  1.  Ni  has  not  been  wholly  removed  if  the  fil.  is  brown  or 
has  black  particles  in  it.  In  that  case  acidify  the  fil.  with  HAc,  boil,  filter,  and 
test  for  Ni.  3.  In  using  aqua  regia  the  smallest  quantity  (usually  a  few  drops) 
that  will  suffice  to  dis.  the  substance  must  be  employed.  The  sol.  may  after- 
wards be  diluted.  Note  the  color  of  Ni  salts.  Sep.  (a)  Ni  and  Co  ;  (b)  Ni  and 
Fe ;  (c)  Ni  and  Cu ;  (d)  Ni,  Cu,  Al ;  (e)  Ni,  Bi,  Sb.  (f)  Test  Ni  with  borax 
bead  (v.  Co  and  Table  G). 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

Ni(OH)2 

pale  green 

i  AmOH, 
'  AmCl,  &c. 

Sol.  NaOH  re-ppts.  slowly 
(violet-blue). 

2 

NaOH 

It 

u 

« 

Insol.  in  NaOH  (ex.).  Un- 

changed in  air. 

3 

Am,CO 

green 

Am2COs  (ex.) 

Sol.  has  blue-green  color. 

4 

NajjCOs 

** 

'  ' 

Xi  ftjvOs  \®^») 

5 

H2S 

NiS 

black 

HN03,  aq.  reg. 

From  neutral  or  alk.  sol., 

not  acid. 

6 

AnijS 

u 

" 

u 

Sol.  (si.)  in  Am2S  (ex.). 

7 

KiFeCye 

NiaFeCyc 

green-white 

AmOH 

8 

KsFeCye 

Ni3Fe2Cyi2 

green-yel. 

AmCl+AmOH+K3FeCy6+ 
Ni",  boiled  =  red  ppt. 

9 

HNa.PO, 

Ni3(P04)2 

green-white 

10 

ZCy 

NiCy2 

y  el.  -green 

KCy  (ex.) 

Dist.  from  Co  by  HC1. 

11 

M,0x 

NiOx 

green 

Leave  24  hours. 

12 

Na2B407  (bead) 

(V.  Table  G.)  Co"  obscures 

test. 

13 

Cl,  Br,  &c. 

Oxidizes  Ni"  to  Ni'". 

14 

H2S,  SO,,  &c. 

Reduces  Ni1"  to  Ni". 

15 

Zn 

Ni 

white 

Also  Cd,  Sn. 

10 

B.B.C.C.  f 

» 

" 

HNO 

Magnetic  powder. 

69.    MANGANESE  (ous),  Mn". 
ANALYTICAL   REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  MnS  (v.  Co,  Ni,  Zn). 
To  sol.  add  AmCl  sol.,  Am2S, 
warm,  filter,  wash  in  hot  H2O 
and  Am2S. 

(1)  MnS 

salmon 

2.  Dis.  MnS  in  HC1  (v.  Co,  Ni). 
To  (1)  add  dil.  HC1,  stir,  filter, 
boil  to  expel  all  H2S,  NH3,  &c. 
(test  a  little  with  PbAc2). 

(S) 

(a)  MnCL 

3.  Ppt.  Mn(OH)2  (v.  Zn). 
To  (a)  add  excess  strong  NaOH 
sol.,  warm. 

(2)  Mn(OH)2 
Mn202(OH)2 

white 
brown 

Supplementary.  —  3.  Mn(OH)2  will  not  ppt.  with  NaOH  if  AmCl  and 
AmO  H  are  present.  Mn(O  H)2  when  pure  is  white,  but  it  rapidly  oxidizes  to 
brown  Mn2O2(OH)2  (variable).  This  should  further  be  tested  by  fusing  it  with 
a  mixture  of  Na2CO3  and  KNO3,  when  bright  green  K2Mn04  and  Na2Mn04  are 
formed,  (a)  See  whether  Mn(OH)2  or  MnS  forms  in  preference  to  the  other. 
Will  these  exist  together  hi  sol. :  (b)  MnCl2  +  ZnS  04  ?  (c)  MnS  O4  +  Cu(N  03)2  ? 
(d)  MnCl2  +  K2Cr04  ?  Sep.  (e)  Mn  and  Ni ;  (f )  Mn  and  As ;  (g)  Mn,  Cu,  Cr ; 
(h)  Pb,  Sr,  Mn. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AmOH 

w  _  SVTT 

Mn(OH)2 

white 

AmCl,  &c. 

Quickly  oxidizes  to  brown 
Mn2O2(OH)2  ;  insoluble  in 
AmCl. 

2 
3 

NaOH 
Am,C03 

MnCOs 

u 

u 

U                  It                  U                  u 

4 

NazCOs 

it 

a 

41 

u          .  u            u            u 

5 

H2S 

MnS 

pink 

HC1,  HAc 

MnS  ppts.  from  MnAc2  (un- 
less HAc  is  present).   Not 

otherwise. 

6 

Am2S 

(t 

(t 

« 

7 

ZiFeCye 

Mn2FeCy6 

white 

HC1 

8 

ZaFeCye 

Mn3Fe2Cyi2 

brown 

Insol.  in  acids. 

9 

HNaaPO* 

Mns(P04)2 

white 

Dil.  acids 

From  AnuMnCL.  etc.  ,  forms 
AmMnP04. 

10 

KCy 

MnCy2 

u 

ZCy  (ex.) 

Darkens  in  air. 

11 

M20x 

MnOx 

" 

Acids 

12 
13 

Na2B407  (bead) 
NaaCOs+KNO,,  1 
ignited  on  Pt  [ 
foil 

Z2Mn04    | 

Na2MnO,  ) 

amethyst 
green 

In  o.  f  .    In  r.  f  .  colorless 
(v.  Table  G). 
(  NajjCOg  bead  (o.  f  .),  same 
{     green  color. 

14 

Cl,  Br,  &c. 

Oxidizes  to  Mn'". 

15 

(H,S),  S02,  &c. 

Reduces  Mn"  to  Mn",  ppts. 
S. 

16 

Zn 

Reduces  Mn'"  to  Mn"  when 

rightly  acidulated. 

17 

HN08+Pb02  (boil) 

HMn04(sol.) 

red 

Seen  on  settling  of  sediment. 

7O.    ZINC,  Zn". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  ZnS  (v.  Co,  Ni,  Mn). 
To  sol.  add  AmCl,  Am2S,  warm, 
filter,  wash  with  hot  H2O  and 
a  few  drops  of  Am2S. 

(1)  ZnS 

white 

2.  Dis.  ZnS  in  HC1  (v.  Co,  Ni). 
To  (1)  add  dil.  HC1,  stir,  filter. 

(S) 

(a)  ZnClo 

3.  Zn(OH)2  sol.  in  excess  NaOH  (v.  Mn). 
To  (a)  add  excess  strong  NaOH 
sol. 

(b)  NaoZnO., 

4.  Ee-ppt.  ZnS. 
Acidify  (b)  with  HAc,  add  Am2S. 

(2)  ZnS 

u 

Supplementary.  — I.  ZnS  is  the  only  white  sulfid,  but  it  must  not  be  con- 
founded with  a  white  ppt.  of  S.  3.  Zn(OH)2  is  not  sol.  in  dil.  sol.  of  NaOH, 
especially  if  boiled.  4.  ZnS  is  ppd.  by  H2S  if  the  sol.  is  acidified  with  HAc. 
Zn  ppts.  these  metals  from  sols,  of  their  salts :  Pb,  Ag,  Hg,  Bi,  Cd,  Cu,  As,  Sn, 
Sb,  Co,  Ni,  Fe.  State  color  of  each  sulfid  in  Groups  II  and  IV  (tabulate). 
What  hydroxids  are  sol.  in  excess  of  NaO  H  ?  Sep.  (a)  Zn  and  Al ;  (b)  Zn  and 
Co  ;  (c)  Zn  and  Mn ;  (d)  Pb,  Fe,  Zn. 

GENERAL  REACTIONS. 


RK-AQT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

I 

AmOH 

ZnOH 

jgel. 
1  white 

AmOH  (ex.) 

Forms  Am2ZnO2.     Boil- 
ing re-ppts. 

2 

NaOH 

u 

u 

NaOH  (ex.) 

All  Zn  salts  are  sol.  in 

NaOH,  except  ZnS. 

3 

Am2C03 

Zn5(OH)6(C08)2 

(( 

AmOH 

V 

4 

N^COs 

tt 

11 

u 

5 

H2S 

ZnS 

white 

From  neutral  sol.   only, 

and  in  part  only. 

6 

Am-jS 

K 

» 

HC1 

Insol.  in  HAc  (v.  Mn"). 

7 

K4FeCyfi 

Zn2FeCy6 

u 

8 

KaFeCye 

Zn3Fe2Cyi2 

yellow 

9 

KCy 

ZnCy2 

white 

KCy  (ex.) 

10 

NaAfcOxMid) 

Hot,  yellow  ;  cold,  white. 

{As  incrustation.  On  cool- 

11 

Na,CO..     / 
B.B.C.C.  \ 

ZnO,  Zn 

yellow 

ing  becomes  white. 
Co(NO3)2   makes   green 

color  on  heating  again. 

71.    GROUP  IV.  — Co,  Ni,  Mn,  Zn. 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

SOL. 

1.  Fpt.  CoS,  NiS,  HnS,  ZnS. 

To  sol.   add  AmCl,  Am2S,  shake, 
warm   (not   boil),   filter  rapidly. 
Pour  on  res.  a  few  drops  Am2S, 
then  wash  with  hot  H2O. 

(1)  CoS,  NiS, 
MnS,  ZnS 

2.  Sep.  Co,  Ni  from  Mn,  Zn. 

To  (1)  in  e.d.  add  dil.    HC1,  stir 
well,  filter  and  wash. 

(2)  CoS,  NiS 

(a)  MnCl2,  ZnCl2 

3.  Dis.  CoS  and  NiS. 

To  (2)  add  at  once  very  little  aqua 
regia.    Evap.  acid,  dil.  ,  add  HAc. 

(S) 

(b)  CoCl2,  NiCl2 

4.  Sep.  Co  from  Ni. 

To  (b)  add  excess  strong  KN02  sol., 
leave  24  hours,  filter. 

(3)KeCo20(N02)10 

(c)  NiCl2 

5.  Final  test  for  Ni. 

To  (c)  add  excess  strong  NaOH  sol., 
boil. 

(4)  Ni(OH)2 

6.  To  separate  Mn  from  Zn. 

Partly  evap.  (a)  to  concentrate  the 
sol.  and  expel  all  NH3,  acidify 
with    HAc,    add    excess    strong 
NaOH    sol.,    shake,    let    stand, 
filter. 

(5)  Mn(OH)2, 
Mn202(OH)2 

(d)  Na2Zn02 

7.  Final  test  for  Zn. 

Acidify  (d)  with  HAc,  add  Am2S. 

(6)  ZnS 

Supplementary.  —  1.  Am2S  (colorless),  not  Am2Sx  (yellow),  must  be  used. 
CoS,  NiS,  etc. ,  oxidize  to  sulfates  in  air.  Hence  filter  rapidly  with  H20  having 
a  few  drops  of  Am2S.  Group  II  metals,  if  not  all  removed,  may  ppt.  here. 
2.  CoS,  NiS  are  dis.  by  strong  hot  HC1,  and  slightly  by  cold.  6.  ZnS,  MnS  will 
ppt.  on  adding  XaO  H  if  any  H2S  is  present.  Mn  will  not  ppt.  with  NaO  H  if 
AmCl  and  AmOH  are  present.  Zn(OH)2  is  sol.  in  excess  of  strong  cold  NaOH 
sol.  only.  Mn  should  be  tested  for  by.  fusing  with  Na2C  03  and  K  N  O3.  (a)  What 
members  of  Group  III  will  Am2S  ppt.  ?  (b)  of  Group  II  ?  (c)  Group  I  ? 


72.    BARIUM,  Ba". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Inaction  of   AraCl.   AmOH    on    Ba    salts 

(v.  Mg). 
To  sol.  add  AmCl  sol.  ,  AmOH. 

(a)  BaCl2 

2.  Ppt.  BaC03  (v.  Sr,  Ca,  Mg). 
To  (a)  add  Am2CO3  sol.,  warm,  filter, 
wash. 

(1)  BaCOg 

white 

3.  Dis,  BaC03  in  HAc  (v.  Sr,  Ca). 
To  (1)  add  little  HAc. 

(b)  BaAca 

4.  Action  o!  K2Cr207  on  BaAc2  (v.  Sr,  Ca). 
To  (b)  add  K2Cr2O7  sol. 

(2)  BaCr04 

yellow 

Supplementary.  —  Has  AmO  H  any  effect  on  sol.  salts  of  Ba  ?  (a)  Sep.  Ba 
and  Mn ;  (b)  Ba  and  Fe'" ;  (c)  Ba  and  Bi ;  (d)  Ba  and  Hg";  (e)  Ba  and  Hg7. 
(f)  What  numbers  of  Group  IV  will  Am2C  O3  ppt.  ?  (g)  Group  III  ?  (h)  Group  II  ? 
(i)  Group  I  ?  What  Ba  salt  is  insol.  in  HC1  (v.  Exp.  100)?  For  what  test  i& 
Ba(OH)2  used?  BaCO8  occurs  free  in  nature.  How  can  other  Ba  salts  be 
made  from  it  ?  (g)  Make  several,  (h)  Test  the  Ba  flame  by  dipping  a  Pt.  wire 
(or  a  splinter)  into  BaCl2  and  holding  it  in  the  edge  of  a  Bunsen  flame. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

I 

NaOH 

Ba(OH)2 

white 

20  H,0,  Acids 

Must  be  very  cone.  sol. 

2 

Am2CO- 

BaCOs 

u 

Acids 

Slightly  sol.  in  AmCl,  aided  by 

XTrt    OA 

AmOH  and  heat. 

4 

.Ma^lsUs 

HNa^O* 

HBaP04 

u 

u 

Also  AmCl  (si.).   Must  be  neu- 

tral or  alkaline. 

5 

M2S04 

BaS04 

It 

350,000  H.O 

One  of  the  most  insol.  of  salts. 

6 

Z2Cr04 

BaCrO« 

yellow 

j  HAc  (si.), 
(  HC1  (warm) 

Re-ppd.  by  AmOH. 

7 

K2Cr207 

(t 

u 

« 

U                 it                 11 

8 

H2SiF, 

BaSiFe 

white 

HC1,  HN03 

C2H2OH  aids  ppn.,    also  stir- 

ring,  standing  and   boiling. 

Sr  not  ppd.  by  H2SiF6. 

9 

AmjOx 

BaOx 

white 

Acids 

From  cone.  sols. 

10 

Flame  test 

jyellow- 
1  green 

Vis.  through  indigo  sol.;  blue- 
green  through  green  glass. 

73.    STRONTIUM,  Sr". 
ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COL. 

SOL. 

1.  Inaction  of  AmCl  and  AmOH  on  Sr  salts 
(v.  Mg). 
To  sol.  add  AmCl  sol.  ,  AmOH. 

(a)  SrCla 

2.  Ppt.  SrC03  (v.  Mg,  Ba,  Ca). 
To  sol.  add  Am2C03  sol.  ,  warm,  filter, 
wash. 

(1)  SrC03 

white 

3.  Dis.  SrC03  in  HAc  (v.  Ba,  Ca). 
Pour  on  (1)  a  little  HAc. 

(b)  SrAc2 

4.  Inaction  of  K2Cr207  on  SrAc2  (v.  Ba). 
To  (b)  add  little  K2Cr2O7  sol. 

(c)  SrAc2 

5.  Ppt.  SrS04  with  Am2S04. 

To  (c)  add  Am2SO4  sol.,  shake  well, 
let  stand,  filter,  test  filtrate. 

(2)  SrS04 

« 

Supplementary.  —  (a)  Test  the  Sr  flame  by  dipping  a  Pt.  wire  (or  a  splinter) 
into  a  Sr  salt,  and  holding  it  in  the  edge  of  a  Bunsen  flame.  Sep. :  (b)  Sr  and 
Ba;  (c)  Group  IV  and  Sr;  (d)  Group  III  and  Sr;  (e)  Group  II  and  Sr; 
(f)  Group  I  and  Sr.  (g)  If  HC1  were  used  instead  of  HAc  (in  3),  would  the 
subsequent  reaction  take  place  just  as  well  ?  (h)  See  whether  you  can  ascertain 
which  is  more  insol.,  SrS04  or  BaS04. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

fApirlo 

1 

NaOH 

Sr(OH)2 

white 

60H20 

From  cone.  sol. 

2 

AniiCO: 

SrCOs 

" 

Acids 

From  neutral  or  alkaline  sol. 

3 

Na2CO;, 

'  ' 

'  ' 

4 

HNa2P04 

HSrP04 

" 

M.  acids 

Partly  sol.  in  AmCl. 

6 

M2S04 

SrS04 

" 

(  500HC1, 
i  7000H20 

Let  it  stand  some  time. 

6 

Am20z 

SrOx 

U 

(  HC1,  HN03, 
(AmCl 

Slightly  sol.  in  HAc. 

7 

K2Cr04 

SrCr04 

yellow 

Acids 

From  cone.  sol. 

8 

Flame  test 

crimson 

Best  with  SrCl2. 

74.    CALCIUM,  Ca". 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COL. 

SOL. 

1.  Inaction  of  AmCl  and  AmOH  on  Ca  salts 

(v.  Mg). 

To  sol.  add  AmCl  sol.,  AmOH. 

(a)  CaCL 

2.  Ppt.  CaC03  (v.  Mg). 

To  (a)  add  Am2C03  sol.,  warm,  filter, 
wash. 

(1)  CaC03 

white 

3.  Dis.  CaC03  in  HAc  (v.  Ba,  Sr). 

Pour  on  (1)  a  little  HAc. 

(b)  CaAc2 

4.  Inaction  of  K2Cr207  on  CaAc2  (v.  Ba,  Sr). 

To  (b)  add  K2Cr207  sol. 

(c)  CaAca 

5.  Action  of  Am2S04  on  CaAcjj  (v.  Sr). 

To  (c)  add  a  little  Am2S04  sol.,  very 
dil. 

(d)  CaAc-j 

6.  Ppt.  Ca  with  Am20x. 

To  (d)  add  AmOH  and  Am20x  sol. 

(2)  CaOx 

u 

Supplementary.  —  Sep.  (a)  Ca  and  Ba;  (b)  Ca  and  Sf;  (c)  Ca  and  Pb; 
(d)  Ca,  Al,  and  Bi.  CaCO3  is  the  most  abundant  source  of  Ca  salts,  (e)  Make 
several  Ca  salts  from  it.  (f)  Test  CaCl2  with  a  strong  sol.  of  Am2S04,  and 
compare  with  SrCl2.  This  will  show  why  very  dil.  Am2S04must  be  used  to  sep. 
Sr  and  Ca.  (g)  Test  the  Ca  flame,  as  in  the  case  of  Sr,  and  compare  the  two. 
(h)  See  whether  CaSO4  or  SrSO4  is  more  sol.;  (i)  BaSO4  or  CaS04. 

GENERAL  REACTIONS. 


RB-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

2 

NaOH 
Am,C03 

Ca(OH)2 
CaCOs 

white 
u 

(  700H20, 
1  AmOH 
Acids 

Solubility  decreased  by  heat. 
Cone.  sol.  only. 
Slightly  sol.  with  AmCl.    Neutral 
or  alkaline  sol. 

4 

NasCOs 

HNa.PO* 

HCaFOi 

u 

u 

5 

MiSC-4 

CaSO« 

(i 

fH20(sl.), 
\  Acids  (si.), 
I  Am2804 

With  dil.  sol.  use  C2H5OH. 

6 

Am20x 

CaOx 

II 

M.  acids 

Insol.   in  HAc,   H20x.     AmOH 
aids  ppn. 

75.    MAGNESIUM,  Mg ". 

ANALYTICAL  REACTIONS. 


BISECTIONS. 

PPT. 

COL. 

SOL. 

1.  Prevent   ppn.  of   Mg(OH)2   and 
MgC03  (v.  Ba,  Sr,  Ca). 
To    sol.    add    AmCl    sol., 
AmOH. 

(a)  (AmCl)2MgCl2 

2.  Inaction  of  Am2C03  on 
(AmCl)2MgCl2  (v.  Ba,  Sr,  Ca). 
To  (a)  add  Am2C03  sol. 

(b)  <AmCl)2MgCl2 

3.  Ppt.  AmMgP04. 
To  (b)  add  HNa2P04. 

(1)  AmMgP04 

white 

Supplementary.  —  Unless  enough  AmCl  sol.  is  present,  AmO  H  ppts.  half  of 
the  Mg  as  Mg(0  H)2.    AmMgPO4  will  not  readily  ppt.  unless  AmO  H  is  present. 

(a)  Verify  the  above  statements.     To  ppt.  AmMgP04  from  very  dil.  sols.,  warm 
gently,  stir  with  a  glass  rod,  and  let  the  sol.  stand  in  a  warm  place  some  hours. 

(b)  Verify  with  dil.  sol.     (c)  Test  action  of  Am2C  O3  sol.  on  MgCl2  sol.     Does 
any  previous  group  re-agent  ppt.  Mg  ?     If  so,  how  may  ppn.  be  prevented  ? 
(d)  Sep.  Mg  and  Al ;  (e)  Mg  and  Fe'";  (f)  Mg  and  Ba ;  (g)  Mg  and  Cu. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

BEMARKS. 

1 

AmOH 

Mg(OH)2 

white 

\  AmCl, 
1  600H,0 

Only  half  is  ppd.  ,  rest  is 
sol.  as  Am2Mg(S04)2- 

(  Acids, 

2 

NaOH 

(t 

u 

UmCl 

3 

NasCOs 

Mg4(C03)3(OH)2 

u 

AmCl 

Var.toMg5(C03)4(OH)2. 

C02  liberated. 

4 

Am2CO: 

Am,MglCO:-:, 

u 

Dil,  HC1 

Variable  with  strength 

of  sol. 

5 

HNa2P04 

HMgF04 

u 

In  cone.  sol.  only. 

6 

HNa^AsOi 

u 

u 

Action  is  like  HNai2PO4. 

7 

(  AmCl+AmOH 
i  +HNaaP04 

AmMgPO* 

(white 
(  cryst. 

(  Acids, 
j  15,OOOH20 

8 

B.B.C.C. 

pink 

Heat,  add  drop  Co(N03)2 

sol.,  heat  again;  gives 

pink  color,  when  cool. 

76.    GROUP  V.  —  Ba,  Sr,  Ca, 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 


PPT. 


SOL. 


1.  Prevent  ppn.  of   Mg(OH)2  and 

MgC03. 

To  sol.  add  AmCl  sol.,  then 
AmOH. 

2.  Ppt.  BaC03,  SrC03,  CaC08. 

To  (a)  add  Am2C08  sol., 
warm,  filter,  wash. 

3.  Final  test  for  Mg. 

To  (b)  add 

4.  Dis.  BaCO,, ,  SrC03,  CaCO ,  in HAc. 

Pour  on  (1)  a  little  HAc  and 
stir  it. 

5.  Sep.  Ba  from  Sr,  Ca, 

To  (c)  add  K2Cr207  sol., 
filter. 

6.  Ppt.  SrC03,  CaC03. 

Alkalize  (d)  with  AmOH,  add 
Am2CO8  sol.,  boil,  filter, 
wash. 

7.  Dis.  SrC03,  CaC08  in  HAc. 

Dis.  (4)  in  little  HAc  and 
dil.  it. 

8.  Sep.  Sr  and  Ca. 

To  (e)  add  very  dil.  Am2S04 
sol.,  shake,  let  stand  2 
hours,  filter,  test  fil. 

9.  Final  test  for  Ca. 

Alkalize  (f)  with  AmOH,  add 
Am20x  sol. 


(1)  BaC08,  SrC03, 
CaC08 

(2)  AmMgP04 


(3)  BaCr04 


(4)  SrCOs,  CaC03 


(a)  BaClg,  SrCl2,  CaCl2, 
(AmCl)2MgCl2 

(b)  (AmCl)oMgCl3 


(c)  BaAco,  SrAcn,  CaAc-: 


(d)  SrAc2,  CaAc2 


(5)  SrS04 


(6)  CaOx 


(e)  SrAcn,  CaAc2 


(f)  CaAc2,  Ca804 


Supplementary. — 1.  AmOH  alone  partially  ppts.  Mg(OH)2.  AmCl  forms 
with  Mg  salts  sol.  (AmCl)2MgCl2,  on  which  Am2CO8  has  no  effect.  A  large 
excess  must  be  avoided.  Mg  really  forms  a  group  by  itself,  with  a  separate 
re-agent.  4.  HAc  is  used,  instead  of  HC1,  as  K2Cr207  sol.  ppts.  Sr,  Ca,  as  well 
as  Ba  from  sol.  in  mineral  acids.  5.  Only  a  little  of  the  sol.  should  first  be 
tested  for  Ba.  If  present,  the  whole  must  be  treated,  but  if  Ba  is  absent,  the 
rest  may  at  once  be  tested  for  Sr  (by  8).  5.  BaCr03  must  be  removed  (by 
repeated  filtration  if  necessary)  to  prevent  interference  with  Sr  test.  6.  SrS  O4 
is  slightly  sol.  hi  K2Cr2O7  sol.,  hence  it  is  better  to  re-ppt.  Sr  and  Ca  as  carbon- 
ates, and  re-dis.  by  HAc  before  adding  Am2SO4.  8.  Very  dil.  Am2SO4  must 
be  used  to  ppt.  Sr,  or  Ca  will  be  thrown  down  with  it,  as  CaSO4  is  sol.  in  400 
pts.  H2O.  The  sol.  of  Am2SO4  should  be  tested  with  Ca  sol.  of  a  given  strength, 
and  if  after  2  hours  no  ppt.  forms  it  is  sufficiently  dilute.  9.  "All  Sr  must  be 
ppd.  before  testing  for  Ca.  Make  separate  sols,  of  SrSO4,  CaSO4,  MgSO4. 
(a)  Try  BaCl2  sol.  with  each,  (b)  Try  SrCl2  sol.  with  each  of  the  last  two. 
(c)  Try  CaCl2  sol.  with  the  last.  Explain  the  results. 


77.    SODIUM,  Na'. 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 


PPT. 


COLOB. 


1.  Ppt.  NaaSiFg  (v.  Am,  K). 

To  a  part  of  sol.  add  H2SiF6  sol. 

2.  Inaction  of  H2Tr  on  Na  salts  (v.  Am,  K). 

To  part  of  original  sol.  add  H2Tr. 

3.  Inaction  of  H2PtCl0  on  Na  salts  (v.  Am,  K). 

To  part  of  original  sol.  add  a  few  drops 
of  H2PtCl6. 

4.  Flame  test  lor  Na  (v.  K). 

Evap.  part  of  original  sol.  to  dryness, 
test  with  Pt  wire  in  outer  edge  of 
Bunsen  flame.  Intercept  flame  with 
blue  glass  (or  indigo  sol.  in  t.t.). 
Hold  sol.  of  K2Cr2O7  in  t.t.  close  to 
Na  flame. 

5.  Spectroscopic  test  for  Na. 

Test  flame  as  above,  using  a  spectro- 
scope, and  compare  with  a  chart  (v. 
Physics). 


(1) 


white 


No  ppt. 


deep  yellow 
colorless 

decolorized 


yellow  lines, 
etc. 


Supplementary.  —  No  ppt.  is  obtained  with  H2SiF6  unless  the  sol.  is  strong, 
hence  this  is  not  a  very  good  test.  What  salts  of  Na  are  sol.  (v.  Table  A)  ? 
Why  should  the  original  sol.  be  used  in  each  case,  e.g.  in  the  flame  test? 
Test  the  action  of  sol.  Na  salts  on:  (a)  AgNO3  sol.;  (b)  Pb(NO8)a  sol.  Since 
Na  salts  are  sol.,  explain  the  results. 


78.    POTASSIUM,  K'. 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

1.  Ppt,  K2PtCl6  (v.  Na). 
To  part  of  sol.  add  a  few  drops  of  H2PtCle. 

(1)  K2PtCl« 

yellow 

2.  Ppt.  HZTr  (v.  Na). 
To  part  of  original  sol.  add  H2Tr  sol.  and 
C2H5OH. 

(2)  HKTr 

white 

3.  Ppt,  K2SiF6  (v.  Am,  Na). 
To  part  of  original  sol.  add  H2SiF6  sol., 
warm,  let  stand. 

(3)  K2SiF6 

u 

4.  Flame  test  for  K  (v.  Na). 
Evap.  a  little  of  original  sol.  ,  test  with  Pt 
wire  in  the  outer  edge  of  a  Bunsen  flame. 
Cover  flame  with  blue  glass  (or  with  t.t. 
of  indigo  sol.). 

red-violet 

5.  Spectroscopic  test  for  Z  (v.  Na). 
Examine  flame  as  above,  using  a  spectro- 
scope, and  compare  with  a  chart. 

blue  lines, 
&c. 

Supplementary.  —  Neither  H2Tr  nor  H2SiF6  will  cause  a  ppt.  from  dil.  sols. 
What  of  the  common  salts  of  K  are  insol.  (v.  Table)  ?  (a)  Use  several  K  salts 
for  the  above  tests,  e.g.  KC1,  KC1O3,  KN03,  etc.  In  which  is  the  flame  test 
most  distinct  ?  For  flame  tests  use  both  solids  and  sols,  (b)  Dist.  by  the  flame 
test  a  mixture  of  NaCl  and  KC1.  (c)  Dist.  K  and  Na  by  HtTr  sol. 


79.    AMMONIUM,  NH4' (or  Am). 

ANALYTICAL  REACTIONS. 


DIRECTIONS. 

PPT. 

COLOR. 

SOL. 

1.  Ppt.  Am2PtCl6  (v.  Na,  K). 
To  a  part  of  the  sol.  add  a  few 
drops  of  H2PtCle.     Evap.  and 
ignite  (1). 

(1)  Amj,PtCl6 
(2)  Pt  (spongy) 

yellow 

2.  Ppt.  HAmTr  (v.  Na,  K). 
To  some  original  sol.  add  H2Tr 
and  C2H5OH. 

(3)  HAmTr 

white 

3.  Generate  NH3. 

To  some  of  original  sol.  (or  solid) 
add  NaOH  sol.,  heat,  and  test 
gas  (odor,  litmus,  HC1). 

(a)  NHS  gas 

4.  Volatilization. 

Heat,  and  ignite  on  Pt  foil. 

No  residue 

5.  Nessler's  test  for  NH3. 

To  part  of  original  sol.  add  one 
or  two  drops  of  Nessler's  sol. 

(4)  NHg2IH20 

brown 

6.  Inaction  of  H2SiF0  on  Am  salts 
(v.  K,  Na). 
To  part  of  original  sol.  add  H2SiF6 
sol. 

No  ppt. 

Supplementary.  —  HAmTr  will  not  ppt.  unless  a  strong  sol.  is  used.     Test 
several  compounds  of  Am  by  3  and  4,  e.g.  AmNOs,  An^Ox,  AmaSO*,  etc. 


8O.    GROUP  VI.  — Na,  K,  Am. 


TESTS. 


RESULTS. 


1.  Test  for  Na. 

(a)  To  part  of  original  sol.  add  H2SiF6  sol. 

(b)  Apply  flame  test  with  Pt  wire. 

(c)  Apply  spectroscope  with  Pt  wire. 

2.  Tests  for  £. 

(a)  To  part  of  original  sol.  add  H2PtCl6. 

(b)  "      "     "        u        "      "    H2Trsol. 

(c)  "      "     "        "        "      "    H4SiF6sol. 

(d)  Evap.  part  of  original  sol.  and  try  flame  test. 

(e)  «•        "    "       "        "      "     "    spectrosc.  test. 

3.  Tests  for  Am. 

(a)  To  part  of  original  sol.  add  H2PtCl6. 

(b)  "      u    "        "        u      "    H2Tr  and  C2H5OH. 

(c)  u     "     u        "        "      "    NaOH  sol. ,  warm. 

(d)  Evap.  part  of  original  sol.  and  ignite. 

(e)  To  part  of  original  sol.  add  a  drop  of  Nessler's  sol. 


Yellow  flame. 
Yellow  lines. 


K2PtCl6. 
HKTr, 
K2SiF6. 
Purple  flame. 
Blue  lines. 


Am,PtCl«. 
HAmTr, 
NH3  gas. 

NHg2IH80. 


81.    BOKATES,  M8BO8, 


TESTS. 


RESULTS. 


1.  Flame  test. 

Mix  a  bit  of  powdered  Na^O?  (or 
other  borate)  with  a  drop  or  two 
of  H2S04.  Dip  a  Pt  wire  (or  glass 
rod)  in  this,  and  hold  it  in  the 
edge  of  a  Bunsen  flame.  The  same 
test  may  be  applied  by  putting  the 
mixture  in  an  e.d.,  stirring  it  with 
a  little  C2H5OH,  and  setting  the 
latter  on  fire ;  or  by  mixing  a  drop 
or  two  of  glycerin  with  it  and  test- 
ing with  the  Pt  wire.  H3B08  gives 
a  green  flame  without  the  use  of 
H2S04. 

2.  Turmeric  test. 

Add  a  very  little  HC1  to  a  sol.  of 
Na2B4O7  till  it  is  just  acidified, 
then  moisten  a  piece  of  turmeric 
paper  with  it. 


A  green  color  is  imparted  to 
the  flame. 


The  color  of  the  paper  is  red- 
brown.  On  drying,  the  color 
becomes  deeper  red. 


Supplementary. — Phosphates,  salts  of  Cu  and  of  Ba,  except  BaS04,  also 
give  a  green  flame,  as  does  C2HsCl  (formed  by  C2HgOH  and  MCI).  In  testing 
for  B,  chlorids  should  first  be  removed  by  AgNOs,  and  also  Cu  by  H2S.  H2S04 
reduces  salts  of  Ba  to  BaS04  (which  gives  no  green  flame),  and  the  flame  of 
phosphates  is  a  very  feeble  green.  H3B  O3  in  sol.  should  be  evaporated,  after 
first  making  alkaline  to  prevent  volatilization. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

I 

AgNOs 

Ag2(BO,)2 

white 

With  normal  borates.    M8B08 

also  give  Ag2O  (brown). 

2 

PbACa 

Pb(B02)2 

t 

3 

Cad: 

Ca(B02)2 

' 

AmCl,  acids 

Not  ppd.  if  dil. 

4 

BaCl2 

Ba(B02)2 

i 

tl                U 

U            It         U      tt 

6 

A12(S04>3 

A1(OH)8 

4 

Acids 

6 

MgCl2 

Mg(B02)2 

< 

AmCl,  acids 

82.    NITRATES,  MNO3. 


TESTS. 


RESULTS. 


1.  Copperas  test  (v.  MN02). 

Mix  in  a  t.t.  a  sol.  of  MN03,  or  sol. 
to  be  tested,  with  a  fresh  sol.  of 
FeSO4.  When  cold,  introduce  into 
the  bottom  of  the  tube,  with  a  glass 
tube  used  as  a  pipette,  a  little 
H2S04. 

2.  Deflagration  test  (v.  MNO2,  MC103). 

Heat  B.B.C.C.  a  very  little  pow- 
dered MNO3;  or  mix  with  pow- 
dered charcoal,  and  put  into  an  i.t. 
enough  to  cover  a  penknife  point. 
Heat  cautiously. 

3.  Red  fumes  test  (v.  MN02). 

Put  into  an  i.t.  very  little  MNO3, 
heat.  Insert  a  glowing  splinter 
into  the  tube  while  heating. 

4.  Free  HN03. 

(a)  Add  a  little  indigo  sol. 

(b)  Put  a  drop  on  the  finger-nail,  or 

dip  a  feather  into  it. 

(c)  Pour  a  little  on  Cu  and  warm  it. 


(FeS04)2NO.     Brown  ring  or 
halo  at  junction  of  liquids. 


Vigorous  deflagration  ensues. 


N02  and  N203  (red) ;  O  (color- 
less).    Splinter  burns. 


Decolorizes,  changing  to  red 

isatin. 
Turns  animal  matter  yellow. 

Bed  fumes  (N02),  green  liquid, 
Cu(N03)2. 


Supplementary.  —  If  a  ppt.  appears  on  adding  H2SO4,  let  it  settle,  then 
decant.  H2SO4  liberates  HNO3  from  nitrates,  and  FeS04  reduces  HN03  at 
the  surface  of  contact  to  N  0,  which  unites  with  FeS  04.  Let  it  stand  an  hour  or 
more  if  necessary.  Heat  decomposes  this  compound  (FeSO4)2NO,  expelling 
NO.  The  depth  of  color  indicates  the  strength  of  nitrate.  Heat  decomposes 
all  nitrates ;  from  those  of  the  alkali  and  alkaline  earth  metals  are  first  formed 
MNO2  and  O,  then  M2O,  O,  N.  Nitrates  of  Ag  and  Hg  reduce  to  the  metal, 
others  to  the  oxid  only.  KNO3  and  NaNO3  show  faint  fumes,  best  seen  by 
looking  down  the  tube  to  a  white  background.  Indigo  is  also  decolorized  by  Cl, 
Br,  etc.  Nitrates  of  Au  and  Sb  are  unknown.  All  nitrates  are  soluble  except 
Bi(N03)3,  which  reacts  with  H2O  and  ppts.  Bi(OH)2N03  (variable),  and  to  a  less 
extent  Hg/,  Hg",  Sn",  Sniv. 


83.    NITRITES,  MNO2. 


TESTS. 


RESULTS. 


1.  Copperas  test  (v.  MNO3). 

Apply  this  as  in  MNO8. 

2.  Bed  fnmes  test  (v.  MN03). 

To  a  little  MN02  add  a  few  drops  of 

H2SO4. 
Test  the  HNO2  formed  with  iodo- 

starch  sol. 
Test  it  also  with  KMn04  sol. 

3.  lodin  test. 

Add  a  few  drops  of  KI  sol.  to  3  or  4 
cc.  H2O,  then  a  few  drops  of  dil. 
H2SO4;  finally  a  little  MN02  sol. 
(or  substance  to  be  tested). 

Test  yellow  liquid  with  starch  sol. 

4.  Nitrate  test  (v.  General  Reactions). 


Same  result  as  in  MNO3,  but 
more  readily  obtained. 

N02    (red    fumes)    copiously 

evolved ;  also  HN02. 
Starch  iodid  (blue)  formed. 

Decolorized. 


HI  first  formed,  then  H20,  and 
I  set  free  by  MN02  (yellow 
color). 

Iodid  of  starch  (blue). 


Supplementary.  —  Indigo  sol.  is  decolorized  by  nitrites,  but  not  by  nitrates 
except  by  the  addition  of  H2S04,  which  forms  HNO3.  Apply  the  test.  All 
nitrites  are  soluble,  but  AgNO2  and  Pb(N03)2  only  slightly.  Hence  this  test 
cannot  be  applied  in  dil.  sols. 


GENERAL  REACTIONS. 


BE-AGT. 

PPT. 

CO  LOB. 

SOLVENTS. 

REMAKKS. 

1 

AgNOs 

AgN02 

white 

\  Acids, 
i  H20  (ex.) 

This  distinguishes  MN02  from 

MNOg. 

2 

Pb(NOs)2 

Pb(N02)2 

u 

it 

u           it           u           a           « 

84.    CHLORATES,  MC1O3. 


TESTS. 


RESULTS. 


1.  Oxygen  test  (v.  MN02,  MN03). 

Heat  a  small  quantity  of  the  solid  in 

at.t. 

Test  the  O  with  a  glowing  splinter. 
Dis.  the  residue  when  cool,  and  test 

for  MCI  with  a  drop  of  AgN03  sol. 

2.  Chlorin  test  (v.  MN02,  MN03). 

To  a  very  little  of  the  powder  in  a 
t.t.  add  with  great  caution  a  few 
drops  of  H2S04. 

3.  Deflagration  test  (v.  MN03). 

Powder  and  heat  B.B.C.C. 

4.  Bleaching  test  (v.  MN02,  MN08). 

To  sol.  of  indigo  add  MC103  sol. ,  and 

heat. 
Mix  sols,  of  MC103  and  H2S03,  and 

add  to  indigo  sol.,  without  heating. 

5.  Silver  nitrate  test  (v.  MAc,  MN03). 

To  sol.  add  a  few  drops  of  AgNO3  sol. 


Melts,  O  escapes,  MCI  remains. 

Re-kindles  vigorously. 
AgCl    (white)    ppts.,    sol.    in 
AmOH. 


C102  (green-yellow,  of  charac- 
teristic odor)  liberated  with 
explosive  violence. 

Deflagrates. 


Turned  red  (isatin). 


No  effect  if  the  MC103  is  pure. 


Supplementary.  —  All  chlorates  are  soluble.  Sb,  Sn,  and  Au  have  no  known 
chlorates.  The  deflagration  of  chlorates  is  greater  than  of  nitrates,  (a)  Test 
this  by  scratching  different  kinds  of  matches.  A  few  drops  of  HC1  added  to  a 
few  crystals  of  MC1O3,  and  heated,  give  C102  and  Cl,  of  characteristic  odor. 
Heat  liberates  O  with  violence  from  chlorates,  but  the  presence  of  certain  oxids 
(e.g.  Mn02)  causes  it  to  be  liberated  more  regularly,  and  at  a  lower  temperature. 
Dist.  (b)  KC103  and  KC1;  (c)  KC103  and  KNO3 ;  (d)  KC1O8  and  KNO2. 


85.    CARBONATES,  M2CO3. 


TESTS. 


RESULTS. 


1.  Lime  water  test, 

To  the  solid  (or  sol.)  add  a  little  dil. 
HC1.  Test  the  gas  with  a  drop  of 
Ca(OH)2  sol.  on  a  s.r.,  or  pass  it 
into  Ca(OH)2  sol.,  or  shake  the 
lime  water  with  the  gas. 

2.  Barium  hydroxid  test, 

Apply  this  hi  the  same  way  as  the 
lime  water  test,  using  Ba(OH)2  sol. 
instead  of  Ca(OH)2. 

3.  Flame  test. 

Put  a  burning  splinter  into  the  gas 
generated,  as  above. 


CO2  gas  (colorless)  is  formed, 
which  ppts.  white  CaCOs 
with  lime  water. 


White  BaCO3  fails,  ppd.  by 
CO2  gas,  and  dissolved  with 
effervescence  by  HC1. 


The  flame  is  extinguished. 


Supplementary.  —  Any  acid  (except  H2S,  H  Cy)  will  act  on  any  carbonate 
and  liberate  C02,  but  with  varying  intensity.  H2CO3  with  a  carbonate  (e.g. 
Na2CO3  or  CaCO3)  forms  the  bicarbonate  (primary  or  acid  carbonate),  as 
HNaC03,  H2Ca(CO3)2.  Most  carbonates  are  insol.  Heat  breaks  up  many  of 
them,  forming  the  metallic  oxid  and  C  02.  CaC  O3  requires  a  red  heat,  and  the 
alk.  carbonates  are  not  decomposed  at  the  temperature  of  the  Bunsen  flame 
(v.  oxalates).  Try  the  action  of  various  acids  on  carbonates,  as:  (a)  HAc; 
(b)  H2Ox;  (c)  H2Tr.  Na,  K,  Mg,  burn  in  C02,  liberating  C.  (d)  Pass  C02 
from  a  gen.  into  lime  water  till  the  ppt.  clears,  then  boil.  Dist. :  (e)  C  O2  and 
SO2;  (f)  CO2  and  H2S ;  (g)  CO2  and  N02;  (h)  M2CO3  and  M2Ox.  Some 
metallic  salts  with  Na^C  O3  sol.  give  the  primary  carbonate,  others  the  secondary, 
and  occasionally  a  basic  salt  is  formed,  as  2PbCO3.Pb(OH)2.  Carbonates  are 
white  in  color. 


86.    SULFIDS,  M2S. 


TESTS. 


RESULTS. 


1.  Acid  test. 

To  the  solid  (or  sol.)  add  a  little  dil. 
HC1  (or  H2S04),  and  warm  it. 
Test  the  escaping  gas  (odor,  PbAc2 
sol.  on  paper). 

2.  Coin  test. 

Put  a  drop  of  water  on  a  silver  coin, 
and  on  this  a  soluble  sulfid  (if  in- 
sol.,  first  fuse  with  Na2CO3).  (V. 
M2S03,  M2S203,  M2S04.) 

3.  Ppn.  tests  (v.  General  Reactions). 


H2S  gas  formed,  with  odor  of 
sewer-gas.  Black,  metallic 
PbS  formed. 


Coin  is  blackened. by  forma- 
tion of  Ag2S. 


Supplementary.  —  All  sulfids,  except  those  of  the  alkalies  and  alkaline 
earths  are  insol.  in  H2O.  Most  are  sol.  in  dil.  acids.  A  few  (FeS2,  HgS,  CoS, 
NiS,  etc.)  are  not  acted  on  by  acids,  except  aqua  regia.  In  such  cases  H2S  may 
be  made  by  nascent  H,  with  the  addition  of  a  little  Zn.  No  sulfid  of  Al  or  Cr 
is  known.  Oxidizing  agents  with  sulfids  tend  to  form  sulfates,  or  to  liberate  S 
and  S02.  (a)  Test  several  with  HN03,  or  aqua  regia.  Metallic  sulfids  (includ- 
ing Am2S)  ppt.  from  sols,  metals  of  the  first  four  groups,  except  Cr  and  Al. 
H2S  ppts.  only  the  first  two  groups. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

PPT. 

COLOB. 

SOLVENTS. 

REMARKS. 

With  H2S  : 

With.  Am2S  : 

1 

Pb(N03)2 

PbS 

PbS 

black 

HotHNOa(dil.) 

2 

AgN03 

Ag2S 

Ag2S 

<( 

u        u         u 

3 

HgN03 

Hg,S 

Hg2S 

u 

aqua  regia 

Warming  changes  to 
HgS  and  S. 

4 

HgCl2 

HgS 

HgS 

u 

U               i( 

First  white,  then  yel- 
low, red,  black. 

5 

BiCla 

Bi2S3 

Bi2S3 

u 

HotHNOaCdil.) 

0 

CdCl, 

CdS 

CdS 

yellow 

((           It            11 

7 

CuCl2 

CuS 

CuS 

(  brown- 
f  black 

u        u         u 

8 

AsCla 

AS2S3 

As2S3 

yellow 

(  Am2S2  (ex.), 
1  Am2C03 

Alkaline  sol.  not  ppd. 
with  H2S. 

9 

SbCls 

Sb,S3 

Sb2S3 

(  orange- 
(  red 

(  Am2Sx  (ex.), 
1  HC1  (hot) 

Ppn.  with  Am2S   is 
imperfect. 

10 

SnCI- 

SnS 

SnS 

j  dark- 
i  brown 

U               11 

11 

FeCls 

none 

FeS+S 

black 

Acids 

12 

CoCl2 

(t 

CoS 

u 

aqua  regia 

AmCl  aids  ppn. 

13 

NiCl2 

« 

NiS 

11 

u         u 

<(           U         U 

14 

MnCl= 

u 

MnS 

pink 

Acids 

Turns   dark  -brown. 
AmCl  aids  ppn. 

16 

ZnCls 

(( 

ZnS 

white 

ii 

AmCl  aids  ppn. 

87.    SULFITES,  M2SO3. 


TESTS. 


RESULTS. 


1.  Acid  test. 

To  the  solid  (or  sol.)  add  a  little  HC1 
(or  dil.  H2SO4),  and  heat  it.  Test 
the  escaping  gas  (odor,  K2Cr2O7 
paper). 

2.  Zinc  test. 

To  the  original  sol.  add  Zn  and  dil. 
H2SO4.  Test  the  escaping  gas 
(odor,  PbAc2  paper). 

3.  Coin  test  (v.  M2S,  M2S2O3,  M2SO4). 

Heat  the  solid  B.  B.  C.  C.  with  Na2C03, 
also  without.  Put  res.  on  Ag  coin 
on  which  is  a  drop  of  water. 

4.  Oxidation  test  (v.  M2S04). 

To  some  of  the  original  sol.  add  a 
little  euchlorin  (or  HN03),  and 
heat.  Test  the  product  with  HC1 
and  BaCl2  sol. 


S02  gas  is  liberated,  reducing 
K2Cr207  to  green  O2(S04)3. 


H2S  is  liberated,  forming  with 
PbAc2  black  PbS. 


Na2S  is  formed,  and  on  the 
coin  black  Ag2S. 


M2S03  is  oxidized  to  M2S04, 
and  ppd.  with  BaCl2  as 
white  BaSO4,  insol.  in  HC1. 


Supplementary.  —  The  alkaline  sulfites  are  freely  sol.  in  water.  Most  others 
are  but  slightly  sol.,  or  are  insol.  Sulfites  are  decomposed  by  acids  (except 
H2C03,  H3B03,  H2S).  (a)  Ppt.  BaS03  with  BaCl2  sol.,  dis.  in  HC1,  filter  if 
necessary,  then  oxidize  fil.  with  aqua  regia,  and  try  to  dis.  ppt.  in  HC1.  Heat 
changes  sulfites  to  M20  and  SO2 ;  also  to  M2SO4  and  M2S.  (b)  Make  the  tests. 
Sulfites  are  reducing  agents,  (c)  Test  action  of  SO2  on  FeCl3  sol.,  then  test  sol. 
for  Fe"  and  Fe'".  (d)  Test  HgCl2  with  S02,  then  test  sol.  for  Hg'  or  Hg". 
(e)  Generate  H  in  a  t.t.,  and  test  the  gas  for  H2S  with  PbAc2  paper,  then  add  a 
few  drops  of  Na2SO3  sol.  and  test  again,  (f)  Bring  together  jets  of  S02  and 
H2S.  (g)  Test  the  bleaching  action  of  S  02  sol.  by  putting  in  it  a  colored  flower, 
or  cambric,  (h)  Test  with  litmus  sol.  (i)  Let  some  S02  sol.  stand  for  a  few 
days  in  an  open  rec.,  and  apply  the  BaCl2  and  HC1  test,  (j)  Try  the  action  of 
SO2sol.  onCaCO3. 

GENERAL  REACTIONS. 


KE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

BaCl> 

BaSO; 

white 

HC1  (dil.) 

(V.  M2S04.) 

2 
3 

AgN03 

Pb(N03)2 

Ag2S03 
PbS03 

u 

u 

HN03  (dil.) 

u 

Boiling  ppts.  dark-brown  Ag. 
Not  blackened  on  boiling  (v. 

M2S203). 

4 

FeCla 

Fe2(SO«)3 

red 

Boiling  forms  green  FeSO4. 

6 

HgCl> 

HgCl 

white 

Boiling  reduces  to  gray  Hg. 

88.    THIOSULFATES,  M2S2O3. 


TESTS. 


RESULTS. 


1.  Bulb-tube  test. 

Heat  the  solid  in  a  tube. 

2.  Acid  test. 

Add  to  the  cone.  sol.  (or  the  solid) 

HC1  (or  H2S04),  warm. 
Test  S02  (odor,  K2CrO4). 

3.  Beduction  test  (v.  M2S03). 

(1)  To  a  sol.  of  starch  and  KI  (made 

blue  by  Cl)  add  a  sol.  of  M2S2O3. 

(2)  To  a  sol.  of  starch  and  KI  (un- 

colored)  add  M2S203  sol.  with 
which  a  little  euchlorin  is 
mixed. 

4.  Coin  test  (v.  M2S,  M2S03,  M2S04). 

Fuse  B.B.C.C.,  put  on  Ag  coin  with 
a  drop  of  H2O. 

5.  Precipitation  tests. 

(V.  General  Reactions.) 


Sublimate  of  H2O  and  S,  and 
liberation  of  S02. 

S  ppts.  (white),  S02  formed. 


Decolorized. 

Uncolored,  as  Cl  has  oxidized 
M2S203  to  M2S04  and  HC1. 


Coin  is  blackened  (Ag2S). 


Supplementary.  —  Thiosulf ates,  if  mixed  in  a  mortar  with  chlorates,  explode 
violently.  They  are  strong  reducing  agents.  They  are  mostly  sol.  in  water, 
except  those  of  Ba,  Pb,  Ag.  Dist. : .  (a)  M2S2O3  and  M2S ;  (b)  M2S208  and 
M2S03 ;  (c)  M2S203  and  M2S04. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

BaCl2 

BaS203 

white 

Dil.  acids 

Acids  ppt.  S  (white). 

2 

AgN03 

Ag2S203 

(t 

Na^Oz  (ex.) 

Boiling  forms  Ag2S  (black).  Forms 

slowly  on  standing. 

3 

PbACa 

PbS203 

t( 

u            u 

Boiling  forms  PbS  (black).  Forms 

slowly  on  standing. 

4 

HgN03 

Hg2S203 

t( 

tt           u 

Boiling  forms  Hg2S  (black).  Forms 

slowly  on  standing. 

5 

FeCla 

FeClo 

Acts  as  reducing  agent. 

6 

CaCl2 

none 

Dist.  from  M2SO3. 

89.    FL.UORIDS,  MF. 


TESTS. 


RESULTS. 


1.  Glass- etching  test, 

(1)  Put  a  little  powdered  CaF2  into  a 

small  lead  dish,  and  mix  with 
enough  H2SO4  to  make  a  thick 
paste.  Cover  the  dish  with  a  piece 
of  glass  (coated  with  wax  if  de- 
sired, and  a  design  scratched  on 
it)  and  let  it  stand  in  a  warm  place 
for  several  hours.  Remove  the  wax 
by  melting,  and  finally  with  a  cloth 
wet  with  alcohol,  naphtha,  or  tur- 
pentine. 

(2)  Mix  a  little  CaF2  with  HKS04,  put 

into  a  small  t.t.,  and  heat. 

2.  Turbidity  test. 

Mix  a  little  CaF2,  Si02  and  H2SO4, 
put  into  a  t.t.  and  heat  it,  mean- 
time holding  in  the  tube  on  a  s.r. 
(or  in  the  loop  of  a  Pt  wire)  a  drop 
of  H20. 

3.  Free  HF  in  sol. 

Dip  a  brush  into  the  liquid  in  a 
leaden  dish,  and  mark  out  a  design 
with  it  on  a  glass  plate,  going  over 
it  several  times.  Avoid  getting  any 
HF  sol.  on  the  flesh. 


The  glass  will  be  etched  where 
exposed  to  the  fumes  of  HF, 
SiF4  being  formed. 


The  tube  will  be  roughened 
(or  etched)  by  the  HF. 


The  water  is  rendered  turbid 
by  the  SiF4  gas,  forming 
H2SiF6. 


The  glass  will  be  etched  as 
above. 


Supplementary.  —  Several  of  the  fluorids  are  soluble.  The  most  important 
compounds  of  F  are  CaF2  and  HF.  The  latter  corrodes  glass,  porcelain,  and  all 
metals  except  Pb,  Pt,  and  Au.  CaCl2  ppts.  CaF2  (transparent,  gelatinous). 
BaCl2  ppts.  BaF2  (white).  CaF2,  which  occurs  in  the  earth  as  fluorite  or  fluor- 
spar and  cryolite,  Na3AlFe,  a  mineral  found  in  Greenland,  are  the  main  sources 
of  F  compounds. 


9O.     CHLOKIDS,  MCI. 


TESTS. 


RESULTS. 


1.  HC1  test. 

Add  H2S04  to  the  solid  in  t.t.,  heat. 
Test  gas  (odor,  color,  NH3). 

2.  Cl  test. 

Mix  the  solid  with  MnO2,  add  H2SO4, 
heat.  Test  gas  (odor,  color,  NH3, 
indigo  paper). 

3.  Precipitation  tests. 

(a)  To  sol.  add  AgNO3  sol.    Expose  part 

to  sunlight,  add  AmOH  to  the  rest, 
then  HNO3. 

(b)  To  sol.  add  HgNO3  sol. ;  then  AmOH. 

(c)  To  sol.  add  Pb(NO3)2  sol.  •  boil  with 

plenty  of  H20. 


1IC1  is  liberated. 


Cl  liberated,  green  -  yellow ; 
AmCl  with  NH3,  indigo  pa- 
per bleached. 


AgCl  (white)  ppts. ;  blackens 

in  light ;  sol.  in  AmOH ;  re- 

ppd.  by  HNO3. 
HgCl  (white)  ppts. ;  blackened 

by  AmOH. 
PbCl2    (white)   ppts. ;   sol.   in 

boiling  H20. 


Supplementary.  —  Most  chlorids  are  soluble.  Except. :  Ag,  Pb,  Hg',  Cu'. 
SbCl3,  BiCl3,  SnCl2  decompose  water,  forming  SbO  Cl,  BiO  Cl,  Sn2O  C12.  H2S  O4 
frees  HC1  from  all  chlorids,  except  HgCl  and  HgCl2  (and  not  much  from  Ag, 
Pb,  Sn  chlorids).  HgCl2  sol.  fails  to  ppt.  PbCl2  from  Pb(NO3)2  sol.  (a)  Test 
the  last  statement.  Dist.:  (b)  MCI  and  MC103  (cautiously);  (c)  MCI  and 
MNO3.  (d)  Take  5&  KC1O3  and  divide  into  2  parts.  Dis.  one  in  H2O  and  add 
AgNO3  sol.  Heat  the  other  a  few  minutes,  then  dis.,  and  add  AgNO3  sol. 
Compare  the  results. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AgN03 

AgCl 

white 

AmOH,  etc. 

(v.  Exp.  49.) 

2 

Pb(N03)2 

PbCl2 

u 

Hot  H20 

(v.  Exp.  48.) 

3 

HgN03 

HgCl 

" 

HN03 

(V.  Exp.  50.) 

91.    BBOMII>S,  MBr. 


TESTS. 


RESULTS. 


1.  Bromin    test. 

Mix  Mn02  with  the  solid,  add  a  little 

H2SO4,  heat. 
Test  the  gas  by  holding  in  it  a  paper 

dipped  in  starch-paste. 

2.  I o do- starch  test. 

Liberate  Br  as  above,  and  hold  in  it 
a  paper  dipped  in  a  mixture  of 
starch-paste  and  KI  sol. 

3.  CS,  test. 

To  the  sol.  add  a  drop  or  two  of  €82 
sol.,  and  a  drop  of  euchlorin,  and 
shake  it. 

4.  Silver  nitrate  test. 

To  sol.  add  a  drop  or  two  of  AgNOs 
sol.  Try  to  dis.  part  of  ppt.  in 
HNO8,  another  part  in  AmOH. 


Br  (red  gas)  is  liberated. 
Colors  starch  yellow  to  orange. 


Br  combines  with  K  in  KI,  lib- 
erates I,  which  forms  blue 
starch-iodid. 


Br  is  liberated  and  absorbed 
by  €82,  which  is  colored 
yellow. 


AgBr,  yellow- white,  ppts.,  in- 
sol.  in  HN03,  slowly  sol.  in 
AmOH. 


Supplementary.  — Bromids  are  soluble,  except  those  of  Ag,  Hg',  Hg",  Cu',  Pb. 
BiBr3  and  SbBr3  need  acidulation.  Dilute  H2S04  acts  on  bromids  to  form 
HBr;  strong  acid  forms  Br.  (a)  To  a  bromid  sol.  add  euchlorin  (very  little), 
and  note  the  color,  (b)  Dist.  MBr  and  MCI.  (c)  Pour  a  little  Br  vapor  into 
starch-paste,  and  shake.,  (d)  Mix  starch-paste  and  KBr  sol.  (very  little),  and 
add  a  drop  or  two  of  euchlorin. 

GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOL. 

REMARKS. 

I 

AgN03 

AgBr 

pale  yellow 

AmOH 

Only  slightly  sol.  in  AmOH. 

2 

PbAc2 

PbBr2 

white 

Hot  H20 

Less  sol.  than  AgCl  in  H2O. 

8 

HgN03 

HgBr 

yellow-white 

KBr 

92.    IODIDS,  MI. 


TESTS. 


RESULTS. 


1.  Starch  test. 

Mix  Mn02  with  the  solid,  add  H2S04, 
heat,  and  test  with  cold  starch- 
paste  (v.  Exp.  40). 

2.  CS2  test. 

Add  to  the  sol.  a  drop  of  CS2  [or 
(C2H5)20],  then  2  or  3  drops  of 
euchlorin  (avoid  excess),  and  shake 
it  well. 


Violet  I  vapor  appears,  which 
colors  starch-paste  blue. 


CS2  dis.  the  I  set  free  by  Cl, 
and  is  colored  violet  at  the 
bottom  of  the  tube.  NaOH 
destroys  the  color,  forming 
Nal  and  NaI03. 


Supplementary.  —  Most  iodids  are  sol. ,  except  Pb,  Hg7,  Hg",  Au.  Sb,  Bi, 
Cu,  Sniv  iodids  need  acidulation,  as  they  react  with  H20.  The  double  iodids 
(KIAgI,  etc.)  are  formed  and  dis.  with  excess  of  KI  with  salts  of  Pb,  Ag,  Hg. 
I  may  be  liberated  from  an  iodid  by  Zn  and  HNOs,  HNO2  being  first  formed. 
Euchlorin  or  bromin  acts  the  same.  Iodids  are  broken  up  by  oxidizing  agents 
more  easily  than  bromids  or  chlorids. 


GENERAL  REACTIONS. 


BE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AgN03 

Agl 

yellow-white 

KCy,  Na2S203 

Insol.  in  HNO3  or  ArnOH. 

2 

Pb(N03)2 

PbI3 

yellow 

NaOH  (ex.) 

Dis.  by  HN03. 

8 

HgNOs 

Hgl 

green-yellow 

HgN03  (ex.) 

u       u          u 

4 

Hg(NOs), 

HgI2 

yellow-red 

Hg(N03)2  (ex.) 

u       it   .      u 

5 

CuSCM-HjSOs 

Cul 

white 

H80  (si.) 

Insufficient  reduc.  agent 

ppts.  I. 

93.    ACETATES,  MC2H3O2  (MAc). 


TESTS. 


RESULTS. 


1 .  Charring  test  ( v.  M2Tr,  M20x) . 

Heat  a  very  little  of  the 
solid  in  a  t.t. ,  take  odor. 

2.  Acetic  acid  test  (v.  M2Tr). 

Add  to  the  solid  (or  sol.) 
H2SO4,  heat,  take  the 
odor,  test  with  litmus. 

3.  Acetic  ether  test. 

Add  to  the  sol.  a  few  drops 
of  C2H5OH  and  H2S04, 
warm,  and  take  odor. 

4.  Ferric  test, 

To  sol.  add  FeCl3  sol. ,  boil. 

5.  Silver  nitrate  test  (v.  MNO3, 

MC108). 

To  a  dil.  sol.  add  AgN03 

sol. 
To  a  strong  sol.  add  AgNOs 

sol. 

6.  Cacodyl  test. 

Heat  with  an  alkali  and 
very  little  As^e  ;  take 
odor. 


Melts,  expels  H2O,  turns  black,  gives  odor 
of  acetone,  C3H6O  (inflammable). 


HAc  is  formed,  having  characteristic  odor, 
and  acid  reaction. 


C2H5Ac  is  formed,  having  characteristic 
odor. 


FeAc3  (red  sol.).    Boiling  ppts._  red-brown 
basic  acetate  of  Fe'". 


No  ppt. 

AgAc  (white)  ppts. 


Cacodyl  oxid  As2(CH3)40  evolved  (intensely 
offensive  odor). 


Supplementary.  — All  acetates  are  sol.,  those  of  Ag  and  Hg'  only  partially. 
No  acetate  of  Au  is  known.  Dist.:  (a)  MAc  and  M2Tr;  (b)  MAc  and  M2Ox. 
(a)  Try  to  make  CH4  in  a  t.t.  by  heating  dry  NaOH  and  an  acetate,  (b)  Test 
the  combustibility  of  the  gas.  (c)  Test  some  vinegar  for  acetic  acid,  (d)  Make 
some  HgAc ;  (e)  AgAc.  (f)  See  whether  HAc  will  dis.  Zn ;  (g)  Fe.  (h)  If  so, 
test  the  product  for  Fe"  and  Fe'". 


94.    CYANIDS,  MCN  (MCy). 


TESTS. 


KESULTS. 


1.  HCy  test. 

Add  to  sol.  a  little  H2SO4  (or  HC1). 
Very  cautiously  take  the  odor  by 
fanning  the  gas  to  the  face  with 
the  hand. 

2.  Fe(CyS)3  test. 

Put  a  few  drops  in  an  e.d.,  add 
equally  Am2Sx,  evap.  to  dryness, 
dis.  in  dil.  HC1,  add  FeCl8  sol. 

3.  Prussian  blue  test. 

To  sol.  add  equally  a  few  drops  of 
NaOH  sol.  and  FeS04  sol.,  shake 
and  warm  it,  add  FeCl3.  Dis.  in 
dil.  HC1  (excess). 

4.  AgN03  test. 

To  sol.  add  a  little  A  gN08  sol.  Pour  off 
liquid,  and  boil  with  HNOg.  If  not 
all  dissolves,  test  liquid  with  HC1. 


HCy  is  formed  (very  poison- 
ous) ;  odor  of  bitter  aim  onds. 


MCyS  is  formed,  sol.  in  HC1, 
giving  red  Fe(CyS)3  sol. 
with  FeClg. 


FeCy2  (sol.  in  MCy  excess), 
Fe(OH)2,  Fe(OH)8  formed, 
soluble  in  HC1,  but  ppg. 
Fe4Fe3Cyi8,  deep  blue. 


AgCy  (white)  ppts.,  sol.  in  hot 
HN03,  re-ppd.  by  HC1. 


Supplementary.  —  Use  great  care  in  experimenting  with  cyanids,  as  they 
are  very  poisonous.  Cyanids  are  insol.,  except  HgCy2  and  those  of  the  alkalies 
and  alkaline  earths  (BaCy2  only  slightly).  The  solutions  are  alkaline.  The 
ppd.  cyanids  are  often  sol.  in  excess  of  the  cyanids,  forming  double  salts, 
(a)  Make  several  by  ppn.,  and  then  dissolve.  Dist. :  (b)  MCy  and  MAc; 
(c)  MCy  and  MN03.  In  the  Prussian  blue  test  the  following  equations  indicate 
the  order  of  changes:  (1)  2MCy+FeSO4  =  FeCy2+M2SO4;  (2)  4MCy+FeCy2= 
M4FeCy6;  (3)  FeS04+2NaOH=Fe(OH)2-f NaaSO4;  (4)  2Fe(OH)2+H20+0= 
2Fe(OH)3;  (5)  2HCl+Fe(OH)2=FeCl2+2H2O;  (6)  3HCl+Fe(OH)3=FeCl3+ 
3H2O;  (7)  4FeCl3+3M4FeCy6=Fe4Fe3Cyi8+12MCl.  The  vapor  of  HCy  is  a 
deadly  poison,  N  H3  or  Cl  inhaled  being  the  antidote.  As  used  in  medicine  the 
acid  contains  only  2%  H  Cy. 


95.    TABTKATES, 


(M2Tr). 


TESTS. 


RESULTS. 


1.  Ignition  test  (v.  M20x,  MAc). 

Heat  in  i.t.     Take  odor,  note  res. 

2.  H2S04  test  (v.  MAc,  M2Ox). 

Heat  in  i.t.  with  little  H2SO4. 

3.  Mirror  test. 

Add  AgNO3  sol.  (to  a  neutral  sol.). 
Almost  dis.  ppt.  with  AmOH,  then 
heat  gently  in  t.t. 

4.  Acetic  acid  test  (v.  MAc,  M20x). 

Add  to  sol.  BaCl2  sol.     Dis.  the  ppt. 

in  HAc. 
Add  to  sol.  CaCl2  sol.     Dis.  the  ppt. 

in  AmCl  sol. 

5.  Potassium  chlorid  test. 

Add  KC1  sol.  and  C2H5OH  to  the  sol., 
stir  with  a  glass  rod. 


Evolves  fumes  (white,  then 
brown),  CO2,  with  odor  of 
burnt  sugar,  and  black  resi- 
due, M2CO3,  C. 

CO,  C02,  S02,  C. 


Ag2Tr  (white)  ppts.    Mirror  of 
Ag  collects  on  the  tube. 


BaOx  is  sol.  in  HAc. 

CaOx  forms,   sol.  hi  NaOH, 
re-ppd.  on  boiling. 


HKTr  (white)  ppts.  from 
strong  sols.  only. 


Supplementary.  —  Only  the  alkali  tartrates  are  freely  soluble,  and  the 
bitartrates  of  the  alkali  metals  are  much  less  so  than  the  normal  ones  (v.  tests 
for  K  and  Am).  Dist.:  (a)  M2Tr  and  M20x;  (b)  M2Tr  and  MN02.  (c)  Make 
H  AinTr.  (d)  Try  the  reducing  action  of  H2Tr  on  K2Cr207  sol.  (e)  See  whether 
CaTr  is  sol. 


96.    OXAL.ATES,  M2C2O4  (M2Ox). 


TESTS. 


RESULTS. 


1.  Ignition  test  (v.  M2Tr,  MAc). 

Heat  the  solid  in  an  i.t.  Test  gas  with 
Ca(OH)2  sol.,  also  combustion  of 
CO.  H2Ox  decomposes  with  very 
slight  charring,  and  without  res. 

2.  Acid  test  (v.  MAc,  M2Tr). 

Heat  the  solid  with  H2SO4  (which 
absorbs  the  H2O). 

3.  Calcium  suliate  test. 

Alkalize  the  sol.  with  AmOH,  add  a 
little  CaS04  sol.  Try  to  dis.  part 
of  the  ppt.  with  HAc,  the  rest  with 
dil.  HC1. 


CO2,  CO,  M2O  form.  On  pass- 
ing the  gas  through  NaOH 
sol.  to  remove  C02,  CO  burns 
with  blue  flame. 


CO2,  CO,  M20  form.  Dil.  HC1, 
HN03  or  H2S04  decomposes 
M20x,  forming  H2Ox. 

CaOx  (white)  ppts. ,  sol.  in  dil. 
HC1  without  effervescence, 
insol.  in  HAc. 


Supplementary.  —  On  igniting  oxalates,  carbonates  and  CO  first  form,  then 
oxids  and  C  02.  Ag2Ox  and  HgOx  (which  easily  decompose  with  heat)  give  the 
metals  as  a  final  product.  Ag20  decomposes  with  explosion,  (a)  Test  several 
oxalates,  first  changing  them  to  Ag2Ox.  At  moderate  temperature  H20x 
sublimes  unchanged,  except  to  give  off  its  water  of  crystallization.  Most 
oxalates  are  insoluble,  except  those  of  the  alkali  metals  and  Cr.  HC1,  HNO8,  or 
H2S  04  forms  H20x  from  its  salts.  Oxalates  are  reducing  agents,  (b)  (test  with 
KMn04),  and  are  almost  all  white  in  color,  (c)  Make  several  oxalates.  (d)  vSee 
whether  H20x  will  react  with  metals,  e.g.  Zn  and  Fe. 


GENERAL   REACTIONS. 


RE-A.GT. 

PPT. 

COLOR. 

SOLVENTS. 

I 

CaCl, 

CaOx 

white 

HC1  (dil.) 

2 

FeSO* 

FeOx 

yellow-white 

3 

AgNO, 

Ag20x 

white 

4 

Pb(N03)2 

PbOx 

n 

NaOH,  HNOS 

97.    SILICATES,  M4SiO4,  M2SiO8. 


TESTS. 


RESULTS. 


1.  Acid  test. 

To  strong  sol.  add  HC1 ;  then  evap. 
Add  HC1,  boil,  decant ;  then  add 
to  res.  NaOH  sol.,  boil. 

2.  Fusion  test  (insol.  silicates). 

Mix  thoroughly  2  pts.  dry  K2C03, 
2  pts.  Na2C03,  1  pt.  finely  powdered 
M4Si04  (e.g.  slate,  etc.),  fuse  thor- 
oughly B.B.C.C.  Pulverize,  add 
H2O,  boil,  filter.  To  fil.  add  HC1, 
boil,  evap.  to  dryness.  Try  to  dis. 
in  boiling  HC1,  then  in  boiling 
NaOH  sol.  The  SiO2  may  also  be 
tested  with  CaF2  and  H2S04  in  a 
leaden  dish  (v.  Exp.  28). 


H4Si04  (gelat.,  white)  formed. 
Heat  reduces  to  Si02,  insol. 
in  HC1;  partially  sol.  in 
NaOH  sol. 

K4Si04,  Na4Si04,  M2O  (M2C03) 
are  formed.  First  two  are 
sep.  by  H2O,  and  changed  by 
HC1  to  H4SiO4,  and  by  heat 
to  SiO2  (gritty);  insol.  in 
HC1,  slightly  sol.  in  NaOH. 


Supplementary.  —  Silicates  are  insol.,  except  those  of  the  alkalies,  which 
are  somewhat  soluble.  Some  are  dis.  by  acids,  but  many  are  not.  SiO2  is 
insol.,  even  in  acids  (except  HF),  and  is  also  infusible  in  the  blow-pipe  flame, 
but  is  fusible  in  the  oxyhydrogen  flame.  There  are  two  varieties  of  silica,  the 
amorphous  and  the  crystalline.  The  former  is  sol.  in  NaOH  or  Na2CO3,  the 
latter  not.  In  a  bead  of  Na2C03  at  very  high  temperature,  B.B.,  SiO2  and  all 
silicates  fuse  to  a  clear  glass.  They  will  not  fuse  in  a  bead  of  HNaAmPO4. 
The  best  fusing  mixture  contains  about  half  each  of  Na2C03  and  K2C03,  the 
mixture  melting  at  a  lower  temperature  than  either  alone.  Test  Si03. 


98.    FERROCYANIDS,  H&FeCy* 


TESTS. 


RESULTS. 


1.  Ferrous  test. 

Add  to  the  sol.  —  acidi- 
fied with  HC1  —  a  few 
drops  of  FeS04  sol. 

2.  Ferric  test. 

Add  to  the  sol.  FeCl3  sol. 


3.  Copper  test. 

Add  to  sol.  CuS04  sol. 

4.  Silver  test. 

Add  to  sol.  AgNO3  sol. 


White  K2Fe2Cye  ppts.,  changing  quickly 
to  blue.     Darkens  by  oxidation. 


Prussian  blue,  Fe4Fe3Cyi8,  ppts.,  sol.  in 
H2Ox  (not  HC1)  to  dark-blue  liquid. 
NaOH  changes  to  red-brown  Fe(OH)3. 

Cu2Fe2Cy6  (chocolate)  ppts.,  insol.  in  HAc. 


White  Ag4Fe2Cy6  ppts. ,  insol.  in  HNO3  or 
AmOH.  Heated  with  HN03  the  ppt. 
forms  Ag3Fe2Cye  (orange-red),  sol.  in 
AmOH. 


Supplementary.  — Ferrocyanids  are  mostly  insol.,  except  those  of  the  alkalies 
and  alkaline  earths  (Ba  slightly).  Ferrocyanids  represent  ferrous  compounds, 
ferricyanids  are  from  ferric  salts.  The  most  important  of  the  former  is 
K4FeCy«,  "yellow  prussiate  of  potash."  Make  several  ferrocyanids  by  the 
following  table. 

GENERAL  REACTIONS. 


RH-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMABKS. 

1 

A1C1, 

FeCy2+Al(OH)8 

white 

NaOH 

Forms  slowly. 

2 

SbCl, 

Sb4Fe3Cyi8 

u 

u 

3 

Bid, 

BuFesCyis 

(( 

u 

4 

CdCl, 

Cd,FeCy6 

(( 

HC1,  NaOH 

5 

CaCl, 

EsGaFeCye 

u 

NaOH 

6 

CoCl, 

CosFeCye 

green 

(t 

Becomes  grad.  gray. 

7 

CuCl, 

CugFeCye 

red-brown 

u 

8 

FeS04 

EsFeFeCye 

white-blue 

u 

Rapidly  changes  from 

white  to  blue. 

9 

FeCls 

K4FesCyi8 

blue 

u 

10 

Pb(N03)2 

Pb,FeCy6 

white 

(4 

11 

MgCl2 

AmjMgFeCye 

« 

U 

With  ammonium  salts. 

12 

MnCl, 

Mn2FeCy6 

u 

NaOH,  HC1 

13 

HgN03 

Hg4FeCy6 

u 

NaOH 

14 

Hg(N03)2 

Hg2FeCy6 

It 

u 

Changes  to  HgCy2  and 

Fe3Fe2Cyi2  (blue). 

15 

NiCl2 

NiaFeCye 

green-white 

u 

16 

AgN08 

Ag4FeCy6 

white 

u 

Changes  to  blue. 

17 

ZnClc 

Zn2FeCy« 

u 

srn 

^  t- 


^ 

SITT. 


.    FEBBICYANIDS, 


TESTS. 


RESULTS. 


1.  Ferrous  test. 

Add  to  some  of  the  sol. 
FeSO4  sol. 

2.  Ferric  test, 

Add  to  some  of  the  orig. 
sol.  FeCl3  sol.  Dilute 
if  necessary. 

3.  Copper  test. 

Add  to  some  of  the  orig. 
sol.  CuSO4  sol. 

4.  Silver  test. 

Add  to  some  of  the  orig. 
sol.  AgNO3  sol. 

5.  Zinc  test, 

Add  to  some  of  the  orig. 
sol.  ZnCl2  sol. 


Turnbull's  blue,  Fe3Fe2Cyi2  ppts.  insol.  in 
acids.     NaOH  decolorizes  it. 


No  ppt.,  but  dark-green  to  brown  color- 
ation. 


Yellow-green 
HC1. 


ppte.,  insol.  in 


Orange  Ag3Fe2Cy6  ppts.,  sol.  in  AmOH, 
not  in  HN03. 


Orange  Zn3Fe2Cyi2  ppts.,  sol.  in  HC1  or 
AmOH. 


Supplementary.  —  Ferricyanids  are  mostly  insol.,  except  those  of  alkalies 
and  alkaline  earths.  Alcohol  does  not  ppt.  the  ferricyanid  of  Na  or  K  from 
sol. ,  and  this  also  dist.  it  from  the  ferrocyanid.  Make  the  test.  K3FeCy«  was 
formerly  called  red  prussiate  of  potash. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

AgN03 

AgsFeCye 

red-brown 

AmOH 

2 

Bid 

BiFeCye 

brown 

3 

CdCl2 

CdsFe2Cyi2 

yellow 

AmOH,  HC1 

4 

CoCla 

Co3Fe2Cyi2 

red-brown 

AmOH 

Blood-red  sol.   with 

AmOH  and  AmCl. 

5 

Cud; 

CusFezCyw 

yellow-green 

6 

FeS04 

Fe3Fe2Cyi2 

dark-blue 

7 

Fed-, 

none 

Green  to  brown  color. 

8 

Pb(NOs)* 

uncertain 

dark-brown 

In  cone.  sols.  only. 

9 

MnCl2 

Mn3Fe2Cyi2 

brown 

10 

HgNOs 

uncertain 

red-brown 

Turns  white  eventually. 

11 

Hg(N03)2 

none 

(V.  M4FeCy6.) 

12 

NiCl2 

NisFezCy^ 

yellow-green 

13 

ZnCls 

ZmFezCyw 

orange 

AmOH,  HC1 

(V.  M4FeCy6.) 

1OO.    SULFATES,  M,SO4. 


TESTS. 


RB80LTS. 


1.  Barium  test. 

To  a  little  of  the  sol.  add  BaCl2  sol, 
decant,  and  to  the  res.  add  dil.  HC1. 

2.  Coin  test  (v.  M2S,  M2S08,  M2S2O3). 

Fuse  some  of  the  solid  B.B.C.C.  (r.f.) 
with  a  mixture  of  Na2C03.  Place 
the  product  on  a  silver  coin  with  a 
drop  of  water. 

3.  Insoluble  sul fates. 

Fuse  1  part  of  the  solid  with  2  parts 
each  of  K2CO3  and  NaC03  (in  Pt 
crucible,  if  no  Ag,  Pb,  or  S  is  pres- 
ent). Dis.  what  of  the  product  will 
dis.  in  H2O,  the  rest,  separately, 
in  HC1.  Test  the  former  for  SO4, 
the  latter  for  M. 

4.  Free  H2S04, 

(1)  Put  a  drop  on  paper,  and  evap.  it 

high  above  a  flame,  or  over  a  water- 
bath. 

(2)  Put  a  few  drops  on  sugar  in  an  e.d. 

and  evap.  over  a  water-bath. 

(3)  Evap.  some  H2S04  nearly  to  dryness, 

and  add  a  little  C2H5OH. 


BaSO*  ppts. ,  which  is  insol.  in 
HC1. 


is  formed,  which  dis.  in 
H2O  and  forms  black  Ag*S 
with  Ag. 


K3S04,  NaaS04,  M2COC  are 
formed.  The  first  two  are 
sol.  in  H2O,  the  last  in  HC1. 
The  former  contains  the 
radical,  the  latter  the  metal 
of  the  original. 


The  paper  is  pulped,  rotted,  or 

charred.    Comp.  with  HC1, 

HN03. 
Greenish -black   substance   is 

formed. 

is  liberated,  which  burns 

with  a  luminous  flame. 


Supplementary.  —  In  the  barium  test  use  dil.  HC1  unless  considerable 
water  is  present  for  strong  HC1  dis.  a  little  BaS04,  and  also  ppts.  BaClj  from 
sol.  What  sulfates  are  insol.?  (a)  Prepare  some  PbSO4,  and  test  it  as  aboT« 
in  3.  (b)  Show  that  PbSO4  exists  in  commercial  H2S04  by  diluting  some  witk 
its  vol.  of  water,  (c)  Make  CuS04,  and  test  it.  (d)  Test  NasSOs  for  trace*  of 
Na^S  O4.  Are  most  sulfates  sol.  or  insol.  ? 


GENERAL  REACTIONS. 


KE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

Bad, 

BaSO< 

white 

400,000  pts.  H,0 

The  only  salt  of  Ba  (exc. 

BaSLFe)  insol.  in  dil.  HC1. 

2 

Pb(NOs), 

PbSO* 

u 

NaOH,  Am  Ac 

C2H5OH  aids  ppn. 

3 

SrCl2 

8rSO« 

t( 

7000  pts.  H20 

Ppts.  slowly  in  dil.  sol. 

4 

CaCl, 

CaS04 

(( 

400  pts.  H20 

No  ppt.  in  weak  sol. 

1O1.    CHKOMATES,  M2CrO4. 


TESTS. 


RESULTS. 


1.  Borax  bead  test. 

Make  a  bead  of  Na2B4O7  or 
HNaNH4P04  with  Ft  wire,  dip 
into  sol.,  fuse  in  either  flame. 

2.  Ppn.  tests. 

Apply  the  first  three  tests  below 
(General  Reactions). 

3.  Hydrogen  diozid  test. 

Acidulate  the  sol.  with  H2SO4,  and 
add  a  few  drops  of  dil.  H2O2  sol. 
Then  add  ether,  and  shake.  This 
will  detect  1  part  of  chromate  hi 
40,000  of  water. 


Glass,  yellow-green  when  hot, 
emerald-green  when  cold. 


A  blue  compound  is  formed 
of  uncertain  composition, 
which  the  ether  dis.  and  car- 
ries to  the  surface  as  a  blue 
liquid. 


Supplementary.  —  Most  chromates  are  yellow,  dichroinates  are  red. 
Bichromates  are  confined  to  the  alkali  metals.  K2Cr2O7,  etc.,  ppt.  normal 
chromates,  e.g.  PbCrO4,  BaCrO4  from  sol.  Pb  and  Ba  salts.  In  both  the 
normal  and  the  dichromates  Cr  is  a  hexad,  in  ic  salts  it  is  a  triad,  in  ous  salts  a 
dyad.  What  other  salts  are  yellow  ?  Acids  change  chromates  to  dichromates, 
alkalies  reverse  this.  Reducing  agents  (nascent  H,  SO2,  H2S)  change  Cr™  to 
Cr'"  chromate  to  chromic  salts. 


GENERAL  REACTIONS. 


RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

1 

Bad, 

BaCrO, 

yellow 

Dil.  acids 

2 

Pb(N03)2 

PbCrO* 

it 

(HN03(sl.), 
f  NaOH  (si.) 

Insol.  in  HAc. 

8 

AgN03 

Ag2Cr04 

dark-red     {f^n^' 

4 

HgN03 

Hg2Cr04 

"           i    HN08(8l.) 

Ppt.  ignited  equals  Cr2Og, 

Hg,  0. 

5 

HgCl2 

HgCr04 

orange 

" 

6 

Bid, 

BiiCCrCWs 

yellow 

" 

7 

CdClt 

CdCrO* 

u 

" 

8 

Acids 

M2Cr207 

red  sol. 

Changed  back  by  alkalies 

to  M2Cr04  (yellow). 

9 

H2S+HC1 

S+CrCls 

green  sol. 

Warming  forms  S02,  ppts. 

Cr2O2Cr04  (brown). 

10 

Am,S 

Cr(OH)s 

green 

Acids 

11 

CAOH+Hd 

Crds 

tt 

On  boiling.     Odor  of  al- 

dehyde. 

102.    PHOSPHATES, 


TESTS. 


RESULTS. 


1.  Molybdate  test. 

To  1  or  2  cc.  of  sol.  add  a  drop  or 
two  of  HN03,  then  add  3  or  4  cc. 
Am2Mo04  sol. ,  and  let  stand. 

2.  Magnesium  sulfate  test  (v.  As,  Mg). 

To  sol.  add  AmCl  sol. ,  AmOH,  MgS04 
sol.,  gently  warm,  stir,  let  stand. 

3.  Iron  test. 

To  sol.  add  a  drop  of  HAc,  excess  of 
NaAc  sol.,  and  1  or  2  drops  of 
FeCl8  sol. 

4.  Cobalt  test  (v.  SiO2,  Al). 

Heat  the  solid  B.B.C.C.,  then  on 
white  infusible  mass  put  a  drop  of 
CoCl2  [or  Co(N03)2]  sol.,  and  heat 
again. 

5.  Silver  nitrate  test. 

To  sol.  add  AgNO3  sol. 


Am3P04.12Mo08  (var.,  yel.) 
ppts.,  sol.  in  M8PO4  (ex.)  or 
in  AmOH. 


AmMgPO4  (white,  crystalline) 
ppts. 


FePO4  (yellowish-white,  gel.) 
ppts.,  sol.  in  FeCl8(ex.). 


Residue  becomes  blue. 


Ag3P04  (yellow)  ppte.,  sol.  in 
HN03. 


Supplementary.  —  All  phosphates  are  insoluble  except  those  of  the  alkali 
metals ;  hence  sols,  of  the  other  metallic  salts  ppt.  phosphates.  Most  phosphates 
are  somewhat  sol.  in  HC1.  If  insol.  in  H20,  they  should  be  dis.  in  dil.  HC1, 
Am  Ac  (made  from  AmOH  and  HAc)  added,  then  FeCl3  till  all  the  phosphate 
is  ppd.  The  fil.  will  now  contain  a  chlorid  of  the  original  metal.  This  test 
applies  specially  to  phosphates  of  Ba,  Sr,  Ca,  Mg.  (a)  Apply  the  test  to  each, 
(b)  Test  bone-dust  in  this  way.  (c)  Test  samples  of  fertilizers.  Phosphates  (and 
also  oxalates)  of  Ba,  Sr,  Ca,  Mg,  if  present,  may  ppt.  with  Fe,  Cr,  Al  by  AmOH. 
To  separate  them  dis.  the  ppt.  in  hot  dil.  HN03,  cool  and  add  excess  NaOH  sol., 
which  ppts.  only  Fe  and  the  phosphates  (or  oxalates).  Dis.  the  ppt.  in  HNO», 
add  H2Tr  and  AmO  H,  which  in  excess  ppts.  the  phosphates  and  oxalates,  die- 
solving  the  Fe.  (For  arseniates  and  arsenites,  v.  Exp.  58.) 


GENERAL  REACTIONS. 


1 

2 
3 
4 

5 
6 

7 

RE-AGT. 

PPT. 

COLOR. 

SOLVENTS. 

REMARKS. 

Co(N08)2 
NiCl2 
BiCL 
Cn(N08)2 
HgNOs 
Hg(NOs)2 
Bad, 

C03(P04)2 
Ni3(P04)2 
BiP04 
Cus(P<>4)2 
HgsPO* 
Hg8(P04)« 
Ba,(PO«)I 

red 

light-green 
white 
blue-white 
white 
(i 

it 

AmOH,  acids 

n        i< 

HC1 
HAc 

HNO 
Acids,  Am  salts 
Dil.  HC1 

Insol.  in  HNO,. 
HgCl2  gives  no  ppt. 

|o 


•pipoi 


•pnnojg 


— r 


B*  •   ^"aT 

Sflfe 

S*»||1 
jj|g'S!ajJ 

II  II  II  II  II  II 


iff 


il 

..S  c-^5o-r 


TABLE  B.— Tube  Reactions. 


Put  into  a  small  i.t.  (or  a  bulb  tube)  a  little  of  the  powder,  and  heat  it. 
liefer  the  results  to  this  table. 


GASES. 

SUBLIMATE,  ETC. 

FU- 
SION. 

RESIDUE. 

INDICATION. 

Red-brown,  NO, 

MNO  „  MNO, 

Yellow-gr.    (rare) 

Cl 

(MCI) 

Red,  Br 

MBr 

Violet,  I                    Black 

MI 

Odor,  NH3  ;    HC1 

tests                        White 

NH, 

Odor,SO,;K,Cr207 

M,S04,  M2SOS> 

test 

M,S20:: 

Odor,H,S;  PbAc, 

test                        Yel.-red,  brown  drops 

X 

MsS 

Odor,    Cy    (flame 

crimson) 

(MCy) 

CO2  ;  Ca(OH)a  test 

M,C03,  M,0x 

CO  (flame  blue) 

M80x 

O  (splinter  test) 

MC103,  MNO,, 

MO, 

NjO     " 

X 

All  finally  vaporizes 

AmNO 

Hot  :    yellow.    Cold  : 

white 

HgCl 

;  White 

X 

HgCU 

White,  As4O0            Cryst.    Heat  and  C  = 

(odor)                         mirror 

AfcOe 

White,  needles 

X 

Sb,0, 

O  (splinter  test) 

Metallic  Hg 

Black,  changing  to  red 

HgO 

Yel.-red-brown  drops 

X 

8 

Hot  :  red.    Cool  :  yel. 

As,Ss 

Red  when  rubbed 

HgI2 

Gray;  white  if  rubbed 

Hg 

Black;  red  if  rubbed 

HgS 

Black,  tarry,  burnt  su- 

gar odor 

M8Tr 

Heavy  white 

White  cryst. 

H,0x 

Black;  odor  acetone 

MAc 

Hot:  red-brown.  Cold: 

light  yellow 

Bi20s 

Hot:  black.   Cold:  red 

Fe208 

Hot:  red-brown.  Cold: 

yellow 

PbO 

Hot:yel.-brown.  Cold: 

yellow 

SnO, 

Hot:  yel.   Cold:  white 

ZnO 

M2C08,  (M20),  (M) 

Org.  cpds.ofNa, 

K,Am,Ba,Sr, 

Ca,Mg 

X 

No  decomposition 

Cpds.    of    alka- 

lies, +  Cl,  NO3 

cpds.    of  alk. 

earths 

TABLE  C.  — Action  with  H2SO4. 


Tut  a  little  of  the  powder  into  a  t.t.,  and  add  a  few  drops  of  H-jSO*.    Ualess 
yiolent  action  ensues  (as  with  K  Cl  O8)  heat  it,  and  observe  especially  the  gas. 


OOIOB  OF  GAS. 

ODOR. 

REFERENCE. 

REMARKS. 

GAS. 

INDICATION. 

Violet 

None 

Exp.  92 

Dark  crystal,  sub- 

I 

MI 

limate. 

Yellow 

CIO, 

"      84 

Substance  deto- 

nates violently. 

C102 

MC10, 

Red-brown 

NO, 

"  82,  83 

N02,  N203 

MNO,,MNOo 

Eed 

Br 

"     91 

Br 

MBr 

None 

HC1 

"     90 

HC1 

MCI 

ti 

Stifling 

"     89 

Etches  glass. 

HF 

MF 

« 

H,S 

"      86 

In  tube  open  at  both 

ends  gives  SO2. 

H,S 

M,S 

White 

SO, 

"      87 

S  not  liberated. 

SO, 

M2S08 

ti 

({ 

"      88 

S  is  liberated. 

a 

M,S,0, 

None 

HAc 

"      93 

HAc 

MAc 

« 

HCy 

"     94 

HCy 

MCy 

K 

CO 

"'    96 

CO 

M20x 

« 

None 

"  10,  101 

Kindles  splinter. 

0 

MO,,  M,Cr04 

ti 

K 

"     85 

White    ppt.    with 

lime  water. 

CO, 

M,CO, 

TABLE  D.  —  Heat  on  Charcoal  (B.B.C.C.), 


With  the  round  end  of  the  forceps  make  a  slight  depression  in  a  piece  of 
•harcoal,  and  put  in  a  little  of  the  powdered  substance.  With  a  mouth  blow- 
pipe blow  the  flame  against  it,  cautiously  at  first,  afterwards  strongly. 


RESULTS. 


INDICATIONS. 


1.    Substance  melts  and  runs  into  the  coal. 

3.  Leaves  white,  infusible  residue. 

Add  to  this  a  drop  of  CoCl2  sol. ,  and  heat  again. 
The  color  may  be : 
Blue, 
Green, 
Pink. 

S.    Coats  charcoal : 

White,  volatile,  garlic  odor,  no  globule. 
44  "        hard,  brittle  globule. 

14       when  cool,  yellow  when  hot,  no  globule. 
44  "       "          "          "       "     globule  malle- 

able, but  difficultly  formed. 

Yellow,  globule  easily  formed,  fusible,  soft,  malle- 
able. 

Yellow  (orange  when  hot),  globule  hard,  brittle. 

Brown  or  red,  no  globule. 

4.  Deflagrates. 

5.  Volatilizes. 

0.    Gives  odor. 

Choking  (SO*). 
Garlic. 


Salts  of  the  alka- 
lies, and  some 
alkaline  earths 


Al,  810., 

Zn 

Mg 


As 
Sb 
Zn 

Sn 

Pb 
Bi 
Cd 

MC10,,  MNO, 
Am 


8  or  MtS 
As 


TABLE   E. 
Heat  on  Charcoal  with  Na2CO8  (B.B.C.C., 


Blow  the  inner  flame  (r.f.)  for  some  time  against  a  mixture  of  the  powdered 
substance,  and  dry,  fine  NaaCOs,  using  charcoal,  as  in  Table  D. 


METALLIC  I 
GLOBULE. 

No 
GLOBULE. 

INFUSIBLE 
POWDER.  | 

COLORED  ! 
MASS. 

SOLID  RESIDUE. 

INCRUSTATION. 

INDICATION. 

X 

White,  brilliant,  malleable, 

In  strong  o.f.  red-brown. 

Ag 

non-oxidizable. 

X 

Hard,  brilliant,  oxidizable, 

B.B.  volatile.   Hot,  orange; 

reddish-white. 

cold,  lemon-yellow. 

Bi 

X 

Red,  malleable  ;  oxidizes  to 

black  ;  green  flame. 

Cu 

X 

Easily  formed,  fusible,  mal- 

Hot,   lemon-yellow  ;   cold, 

leable,  oxidizes  to  yel. 

sulfur-yellow;  vol.  B.B.  ; 

O  flame  blue. 

Pb 

X 

White,  malleable,  difficultly 

Hot,   yellow;    cold,   white 

formed,  easily  oxidized. 

near  assay;  non-vol. 

Sn 

X 

White,  volatile;  light-blue 

flame  ;  garlic  odor. 

As 

X 

Red-brown    (like    peacock 

feather)  ;  vol.  B.B, 

Cd 

X 

(x) 

White,  brittle,  oxidizable. 

Hot,  yel.  ;  cold,  blue-white; 

vol.  B.B.  pale  green. 

Sb 

X 

Hot,   yellow;  cold,  white. 

With  Co(N08)2  green. 

Zn 

X 

Infusible  magnetic  powder, 
white,  gray,  black. 

Fe 

X 

It                 It                 tt                 it                 It 

Co 

X 

tt                  It                 It                 It                 tt 

Ni 

X 

Yellow  mass. 

Cr 

x     Green       " 

Mn 

TABLE  F.  —  Flame  Reactions. 

Fuse  one  end  of  a  Pt  wire  into  a  short  glass  tube.  Hold  the  wire  in  the 
outer  edge  of  a  Bunsen  flame  till  the  latter  loses  the  yellow  color  at  first 
imparted.  Moisten  the  wire  with  H2O  or  HC1,  and  dip  it  into  a  little  of  the 
salt,  then  hold  it  again  in  the  flame,  noting  the  color.  Clean  the  wire  with  H  Cl 
and  the  flame. 


FLAME  COLOR. 

REMARKS. 

INDICATION. 

1.  Violet 

Seen  through  blue  glass  looks  red- 

violet  ;  otherwise  Na  obscures  it. 

E 

2.  Bluish 

As 

3.  Blue 

Pb 

4.  Blue-green 

Moistened  with  H2S04. 

M3P04 

5. 

First  blue,  then  green. 

Cu,  espec.  CuCl2 

6.  Yellow-green 

Moistened  with  H2S04. 

MsB03 

7. 

"    HC1. 

Ba 

8.  Greenish 

Very  slight  color. 

Sb 

9.  Bronze-green 

"     evanescent. 

MNO- 

10.  Orange-yellow 

Blue  glass  obscures  the  color. 

Na 

11.  Orange-red 

Obscured  by  Ba. 

Ca 

12.  Crimson 

"         "    " 

Sr 

TABLE  G.  — Bead  Reactions. 

Make  a  loop  in  the  end  of  a  Pt  wire  (Fig.  38,  Exp.  45),  moisten  and  dip  it 
into  some  powdered  borax,  then  hold  it  in  the  flame ;  repeat  till  you  have  a 
glass  bead  filling  the  loop.  Test  a  weak  sol.  (or  the  smallest  bit  of  powder)  by 
bringing  the  bead  in  contact  with  it,  then  blowing  the  flame  against  it  with  a 
blowpipe. 


OXIDIZING  FLAME  (o.f.,  outer). 

REDUCING  FLAME  (r.f.,  inner). 

INDI- 

CATION. 

Hot. 

Co/d. 

Hot. 

Cold. 

Blue 

Blue 

Blue 

Blue 

Co 

Yellow-red 

Green 

Green 

Green 

Cr 

Green 

Blue-green 

Colorless 

Red-brown 

Cu 

Yellow-red 
Violet 

Yellow 
Violet 

Bottle-green 
Colorless 

Bottle-green 
Colorless 

Fe 
Mn 

l( 

Red-brown 

Gray,  cloudy 

Gray,  cloudy 

Ni 

TABLE  H.  —  Aci€l  Radicals  — Resume. 


SALTS. 

f 

w 

BaCl2+HCl. 

s 

AgNO8+HNO8. 

OTHER  RE-AGENTS  AND  RESULTS. 

For  further  explanation,  v.  Exps.  81-102.  —  Abbrevi- 
ations :  b.  black,  bl.  blue,  br.  brown,  ch.  chocolate, 
d.  dark,  g.  green,  1.  light,  o.  orange,  r.  red,  v.  violet, 
w.  white,  y.  yellow. 

M2S04 

w. 

W. 

(w.) 

Pb(N03)2:  w.     SrCl2:  w.    B.B.C.C.  with  Na2C03 

on  Ag:  b. 

M2S03 

w. 

w. 

BaCl2  +  HC1  +  Cl  :    BaS04.     HC1  :    S02    [odor, 

K2Cr207:  g.]. 

M2S203 

w. 

w. 

BaCl2+HCl:  S.  HC1:  S+S02  [odor,  KoO2O7:  g.]. 

M2C03 

w. 

w. 

HC1:  C02  [Ca(OH)2:  w.].     Heat:  (M2O,  CO2).^  ' 

M2Cr04 

i-y. 

d.-r. 

Pb(N03)2:  y.     HgN03:  d.-r.    HgClo:  o.    BiCl3:  y. 

Cd(NO3)2:  y.   H2S:  y.  Acids:  r,  which  y.  by  alk. 

M3POi 

w. 

i-y. 

AmCl+AmOH+MgS04:  w.    HN03+Am2MoO4: 

y.    B.B.C.C.  +Co(N03)2:bl. 

M3As04 

w. 

ch.- 

H2S,  warm  :  y.     AmCl  +  AmOH  -f  MgS04  :  w. 

br. 

B.B.C.C.:  As  [garlic  odor,  white  fumes]. 

M3As03 

w. 

y.-w. 

H2S+HCl:y.   CuS04  (neutral):  g.  K2Cr04+heat: 

g.    KMnO4:  decol.    C.C.  +  heat,  t.t.  :  mirror. 

M3B03 

w. 

w. 

H2SO4,  Pt  wire:  green  flame.     Turmeric  paper  + 

H3B03  :  br.     H2SO4+  C2H5OH  :  green  flame. 

M,0x 

w. 

w. 

SrCl2:  w.     CaCl2:  w.  [sol.  in  HC1,  insol.  in  HAc]. 

Heat:  CO,  CO2,  M2C03,  M2O  or  M,  no  char- 

ring.    H2SO4:  effervesc.,  CO2. 

M2Tr 

w. 

w. 

CaCl2:  w.   [sol.  in  NaOH].    KC1:  w.    Heat:  chars 

M:;SiO, 

w. 

i-y. 

[odor].     AgN03+AmOH:  Ag  mirror. 
HCl+heat:  Si02.    Na2C03  bead:  effervesc.,  forms 

glass.     HNaAmP04  bead:    insol.   B.B.C.C.+ 

HC1,  evap.  :  SiO2,  sol.  in  NaOH. 

MN02 

w. 

w. 

H2S04:    N02.      HAc+KMn04:    decol.     HAc  + 

AgN03:  w.     HAc  +KI+  starch:  bl. 

MF 

w. 

H2S04+heat:    etches  glass,  makes  H20  turbid. 

HKS04  +  heat  :   green  flame. 

MCI 

w. 

W. 

H2S04:   HC1.     H2SO4+Mn02:  Cl.     AgNX)3:  w. 

[sol.  in  AmOH,  action  of  light].    Pb(N03)2:  w. 

MBr 

y.-w. 

y.-w. 

PbAc2  :  w.     CS2  +  Cl  :   y.     H2S04  +  Mn02  :   Br 

[starch,  KI+  starch]. 

MI 

y.-w. 

y.-w. 

Pb(N03)2:  y.     HgN03:  y.-g.    HgCl2:  y.-r.    CS2+ 

Cl  :  v.     H2SO4  +  MnO2  :  I  [starch  test]  . 

MCy 

y.-w. 

y.-w. 

CuS04:    y.-g.      Co(N03)2:   w.-br.     NiClo  :   y.-g. 
H2S04:  HCy  [odor  cautiously].    KOH+FeSO4 

+  HCl:bl. 

M,S 

b. 

b. 

HC1:  H2S  [odor,  PbAc2].    B.B.C.C.  on  Ag:  b. 

M4FeCyo 

w. 

g-br 

FeCl3:  bl.     FeS04:  bl.-w.    CuSO4:  br.-r. 

M3FeCvfi 

0. 

o. 

FeCl3:  r.-br.     CuSO4:  g.-y. 

MN03 

Heat,i.t.:O,NO2.  B.B.C.C.:  deflagrates.  H2S04: 

N02.    FeS04+H2SO4:  r.-br.    H2S04  +  indigo 

sol.:  decol. 

MC10: 

HCl+heat:  g.-y.    Heat,  i.t.  :  O.    H2S04  (very  lit- 

tle) :  C1204  [y.  gas]  . 

MAc 

Heat:   blackens    [odor].     H2S04  :    HAc   [odor]. 

H2SO4  +  C2H5OH  :    C2H5Ac    [odor].      FeCl3, 

boil:  r. 

TABLE  I.  — Acid  Radicals. 

Arranged  according  to  convenient  method  of  detection. 

1.  Flame  {  H3B03  (M3B03+H2S04). 

f  (with  heat)  {  MN03. 

2.  Gas  J    (with  acid)  {  MN02,  MC103,  M2C03,  M2S,  M2S03,  M2S203. 

i  (with  heat  and  acid)  {  MF,  MCI,  MBr,  MI,  MAc,  MCy. 

o     -a^     P  j   (with  heat)  {  M2Tr,  M20x, 

e  )  (with  heat  and  acid)  {  M4Si04  (M2Si03). 

f  (iron-cyanids)  {  M4FeCy6,  M3FeCy6. 
4.    Precipitate  1   (insoluble)  {  M2S04. 

L  (unclassed)  {  M2Cr04,  M3P04,  M3As04,  M3As03. 


COMPLETE  ANALYSIS. 

In  making  a  complete  analysis,  i.  e.  analysis  for  the  metal  and  acid  radical, 
the  following  order  should  be  observed,  and  the  pupil  should  begin  with  only 
a  single  substance,  such  as  Pb(N03)2,  FeCl3,  etc.,  and  should  make  a  careful 
record  under  each  head. 

1.  External  properties:  Color,  luster,  form  (crystalline  or  amorphous),  taste, 
odor,  deliquescent,  efflorescent,  etc. 

2.  Heat  in  glass  tube  (v.  Table  B). 

3.  Heat  with  H2S04  (v.  Table  C). 

4.  Heat  B.B.C.C,  (v.  Table  D). 

5.  Heat  B.B.C.C.  NaaCO-j  (r.f.)  (v.  Table  E). 

6.  Apply  flame  test  (v.  Table  F). 

7.  Apply  Borax  bead  test  (v.  Table  G). 

8.  Test  solubility  (v.  Table  A). 

9.  Test  for  Metals  (aqueous  analysis)  (v.  Exps.  48-80). 

10.  Test  for  Acid  radicals  (v.  Tables  H,  I). 

11.  State  conclusion  as  to  composition. 


UNIVERSITY  OF  CALIFORNIA  LIBRARY 
BERKELEY 

Return  to  desk  from  which  borrowed. 
This  book  is  DUE  on  the  last  date  stamped  below. 


<     2   1948 
23May'58  D 


100m-9,'47(A5702sl6)476 


